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# find [ohâˆ’] of a 0.33 m methylamine (ch3nh2) solution. (methylamine has a kb value of 4.4Ã—10âˆ’4.)

what is the pH of a 0.10 M solution of methylamine (CH3NH2, kb= 4.4*10^-4) at 25 degree C?
23,742 results
chemistry
CH3NH2(aq)+H2O(l)=>CH3NH3+(aq)+OH-(aq) Kb=4.4 x 10^-4 Methylamine, CH3NH2, is a weak base that reacts with water according to the equation above. A student obtains a 50.0 mL sample of a methylamine solution and determines the pH of the solution to be

asked by ashdawg on April 4, 2013
AP Chemistry
CH3NH2(aq)+H2O(l)=>CH3NH3+(aq)+OH-(aq) Kb=4.4 x 10^-4 Methylamine, CH3NH2, is a weak base that reacts with water according to the equation above. A student obtains a 50.0 mL sample of a methylamine solution and determines the pH of the solution to be

asked by Christina on May 2, 2013
chemistry
What ratio [CH3NH3+]/[CH3NH2] is needed to prepare a buffer solution with a pH of 8.60 from methylamine, CH3NH2, and methylammonium chloride, CH3NH3Cl? Kb of CH3NH2 = 3.7e-4.

asked by Kasey on October 6, 2011
Chemistry
A few questions I don’t really get and need to see the work for A 50.0 mL sample of 0.55 M benzoic acid, C6H5COOH, a weak monoprotic acid, is titrated with 0.51 M NaOH. Calculate the pH at the equivalence point. Ka of C6H5COOH = 6.5 multiplied by 10-5.

asked by Dubs on April 22, 2010
Chemistry
A solution is prepared by diluting 65.0 mL of 0.175 M methylamine, CH3NH2, to a total volume of 225 mL. Calculate the pH of the diluted solution. Kb (CH3NH2) = 4.40 x 10-4

asked by Mallory on June 26, 2011

Analytical Chemistry
Calculate the pH at the equivalence point for the titration of 0.160 M methylamine (CH3NH2) with 0.160 M HCl. The Kb of methylamine is 5.0× 10–4. Methylamine is a weak base and reacts with HCl to give the methylammonium ion. HCl + CH3NH2 CH3NH3^+ + Cl^-

asked by Sam on February 27, 2013
CHEIMSRTY
Methylamine (CH3NH2) forms hydroxide ions in aqueous solution. Why is methylamine a Brønsted-Lowry base but not an Arrhenius base? I need help on this question. Please explain this to me!

asked by Sean on March 14, 2010
CHEMISTRY
Methylamine (CH3NH2) forms hydroxide ions in aqueous solution. Why is methylamine a Brønsted-Lowry base but not an Arrhenius base? I need help on this question. Please explain this to me!

asked by Sean on March 14, 2010
chemistry
what is the pH of a 0.10 M solution of methylamine (CH3NH2, kb= 4.4*10^-4) at 25 degree C?

asked by Crystal on November 28, 2012
chemistry
what is the pH of a 0.10 M solution of methylamine (CH3NH2, kb= 4.4*10^-4) at 25 degree C?

asked by Crystal on November 28, 2012
Chemistry
Find the pH of a buffer that consists of 0.82 M methylamin (CH3NH2) and 0.71 M CH3NH3Cl (pKb of methylamine (CH3NH2) = 3.35.) I keep getting 3.41, but it says that it’s wrong…

asked by Edward on March 3, 2013
Chemistry
What is the pH of a solution that is 0.10 M CH3NH2 (methylamine) and 0.15 M methylammonium chloride?

asked by steve on February 24, 2011
what is the pH of a solution that is 0.200 M in methylamine, CH3 NH2 CH3NH2+ H20 CH3NH3+ + OH- Kb= 4.2 x 10 ^-4

asked by shanice on November 9, 2010
Chemistry!!
Calculate the pH at the equivalence point for the titration of 0.180 M methylamine (CH3NH2) with 0.180 M HCl. The Kb of methylamine is 5.0Ã— 10^â€“4.

asked by Sarah on May 11, 2012
Chemistry
Calculate the pH at the equivalence point for the titration of 0.180 M methylamine (CH3NH2) with 0.180 M HCl. The Kb of methylamine is 5.0× 10–4.

asked by Mandy on December 5, 2013

Chemistry
Calculate the pH at the equivalence point for the titration of 0.200 M methylamine (CH3NH2) with 0.200 M HCl. The Kb of methylamine is 5.0× 10–4.

asked by KB on March 11, 2013
chemistry
Calculate the pH at the equivalence point for the titration of 0.210 M methylamine (CH3NH2) with 0.210 M HCl. The Kb of methylamine is 5.0×10−4.

asked by Anonymous on March 26, 2018
CHemistry
Calculate the pH at the equivalence point for the titration of 0.140 M methylamine (CH3NH2) with 0.140 M HCl. The Kb of methylamine is 5.0× 10–4.

asked by Francesca on March 10, 2015
Chemistry HELP
A solution of gaseous methylamine, CH3NH2, turns red litmus blue. Write the equation and explain this observation.

asked by Tarkan on December 22, 2010
Chemistry
I am very confused about how to start this problem: A 29.8 mL sample of 0.354 M methylamine, CH3NH2, is titrated with 0.231 M hydrochloric acid. The pH before the addition of any hydrochloric acid is ?. The Kb of methylamine is 4.2×10^-4

asked by Dan on April 28, 2012
Chemistry
A) Determine the pH of a 0.98 x 10^-2 mol L solution of hydrocyanic acid (HCN) Ka = 4.0 x 10^-10 B) What is the pH of a 0.243mol L solution of methylamine? (pKb for CH3NH2 = 3.30) C) determine the pH of a buffer solution of Na2CO3 (pkb = 3.68, 0.125 M) and

asked by Jake on June 3, 2013
General Chemistry
1,When aqueous sodium hydroxide is added to a solution containing lead(II) nitrate, a soHowever, when additional aqueous hydroxide is added the precipitate redissolves forming a soluble [Pb(OH)4]2–(aq) complex ion.lid precipitate forms. 2,The Ksp of

chemistry
Consider a buffer solution consisting of CH3NH3Cl and CH3NH2. Which of the following statements are true concerning this solution? (Ka for CH3NH3+ = 2.3 x 10 -11). 1. A solution consisting of 0.1 M CH3NH3Cl and 0.1 M CH3NH2 would be a more effective buffer

asked by bekah on March 25, 2014
Chemistry
I’m trying do this question: 0.10 mol/L hydrochloric acid is titrated with 0.10 mol/L methylamine, CH3NH2. Calculate the pH of the equivalence point. I’m having trouble with the equation… How do you know what HCl + CH3NH2 will produce? Is there a rule or

chemistry
MF16014: What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M methylamine wiht 25.00 mL of 0.10 M methylammonium chloride? Assume that volumes are additive and that Kb = 3.70 x 10-4 for CH3NH2. how do i go about this question? If you know how

asked by joe on May 1, 2007

chem 2
methylamine is a weak base. calculate the pH of a .025 M solution of methylamine.

asked by timmy on November 4, 2014
Organic Chemistry
what is the name of the amide that is formed by the following reaction: Butanoic acid + Methylamine? – CH3CH2CH2COOH + CH3NH2 —> product + H2O? i put n-methylbutyramide and they counted it wrong.

asked by Tina on January 21, 2010
Chemistry
A 119.2mL sample of 0.105M methylamine (CH3NH2, Kb=3.7*10^-4) is titrated with 0.255M HNO3. Calculate the after the addition of each of the following volumes of acid. 49.1mL and 73.6mL. Please help.

asked by Melissa on February 6, 2011
AP Chemistry
In the titration of 77.5 mL of 1.0 M methylamine, CH3NH2 (Kb = 4.4 10-4), with 0.38 M HCl, calculate the pH under the following conditions. (a) after 50.0 mL of 0.38 M HCl has been added (b) at the stoichiometric point

asked by Bill on February 7, 2012
chemistry
0.10 M methylamine (CH3NH2) kb= 4.38e-4 calc the percent ionization so i did the ICE table to find that x=6.26e-3 and then i divided by .1 and then multiplied by 100. but i got the wrong answer whats did i do wrong?

asked by Spencer on February 14, 2009
Buffer solution
Solve an equilibrium problem (using an ICE table) to calculate the pH. a solution that is 0.205 M in CH3NH2 and 0.110 M in CH3NH3Br. i used th Ka of CH3NH2 and set up the problem as Ka=[H3O][CH3NH2]/[CH3NH3Br], but that was wrong. So i switched the

asked by Kyle on March 27, 2010
CHEMISTRY!!!=0
Determine pH of each solution: b) 0.20 M CH3NH3I I did…. CH3NH3^+ +H2O -> CH3NH2 + H3O^+ 0.20 —————0————–0 0.20-x————–x————x so i got… ? =x^2/0.20-x i looked up in the back of the book and found the Kb of CH3NH2 to

asked by ALISON on March 1, 2012
organic chemistry
What is the complete reaction mechanism for the reaction between butanone and methylamine (CH3NH2) with the reaction buffered at a pH of 3.5 and heated.

asked by Jenn on July 28, 2014
Chemistry
At 25°C, the methylaminium ion, CH3NH3+, has a Ka of 2.0 x 10–11. Which of the following is the pH of a 0.15 mol L–1 solution of methylamine? i tried out two methods because im not getting the right answer: H20 + Ch3Nh2 -> CH3NH3+ + OH- I made a

Chemistry
I am stumped on this one…Please help!!! Write a balanced base ionization reaction for methylamine (CH3NH2) in water. Identify all species as acids and bases and identify the conjuate acid-base pairs.

asked by Nathan on November 19, 2011

chemistry
What is the [CH3NH3+] of a solution which is 0.1003 M in CH3NH2 and 0.1204 M in CsOH? CH3NH2(aq) + H2O(l) « CH3NH3+(aq) + OH−(aq)

asked by Andy on May 6, 2014
Chemistry
NEWW- 0.10 M methylamine (CH3NH2) kb= 4.38e-4 calc the percent ionization so i did the ICE table to find that x=6.62e-3 (that was a typo the first time) and then i divided by .1 and then multiplied by 100. but i got the wrong answer whats did i do wrong?

asked by Spencer on February 15, 2009
Chemistry
A 100.0 mL of 0.200 M methylamine, CH3NH2, is titrated with 0.100 M HCl. Calculate the pH after 70.0 mL of 0.100 M HCl has been added.

asked by Donna on November 14, 2009
chemistry
Which of the following statements is true regarding the Lewis structure for methylamine, CH3NH2? a) There will be an unshared pair of electrons on the nitrogen atom. b) There will be three covalent bonds to the carbon. c) Nitrogen will form a double bond

asked by Sawyer on September 9, 2010
college chemistry
Calculate the [CH3NH3+] of a 7.02×10-3 M solution of the weak base CH3NH2 (make an approximate calculation assuming that initial concentration is equal to the equilibrium concentration). Round your answer to 3 significant digits. CH3NH2 + H2O = CH3NH3+ +

asked by sparkle on October 26, 2010
Chemistry
NH3 and CH3NH2 have Kb values of 1.8 x 10-5 and 5.0 x 10-4, respectively; which of the following statement(s) is (are) CORRECT? (i) CH3NH2 is a stronger base than NH3. (ii) the conjugate acid of CH3NH2 is a stronger acid than the conjugate acid of NH3.

asked by A.A on November 1, 2008
college
NH3 and CH3NH2 have Kb values of 1.8 x 10-5 and 5.0 x 10-4, respectively; which of the following statement(s) is (are) CORRECT? (i) CH3NH2 is a stronger base than NH3. (ii) the conjugate acid of CH3NH2 is a stronger acid than the conjugate acid of NH3.

asked by A.A on November 1, 2008
Chemistry Help
The most effective buffer solutions have equal concentrations of salt and acid (or base). Find the pH of a buffer solution with equimolar concentrations of: (a) HCOOH and NaCOOH (Ka = 3.5 x 10-4 for HCOOH) (b)CH3NH2 and CH3NH3Cl (Kb = 3.7 x 10-4 for

asked by Luke on February 23, 2017
Chemistry
In one experiment, 50.0ml of 0.10M CH3NH2, is mixed with 20.00ml of 0.10 M CH3NH3Cl. The kb of CH3NH2 is 3.70*10^-4. a) write the chemical reaction for the equilibrium which becomes established, using H2O as a reactant. b)Write the net-ionic equation that

asked by James on February 27, 2010
chem
Indicate whether the pH increases, decreases, or remains the same when each of the following is added. (CH3NH3)Cl to a solution of CH3NH2 pyridinium nitrate, (C5H5NH)(NO3) to a solution of pyridine, C5H5N sodium formate to a solution of formic acid how do

asked by hannah on March 18, 2013

Chemistry
What will the pH be if 15 mL of 0.1 M HCl are added to the buffer obtained by mixing 70 mL of 0.5 M CH3NH2 and 30 mL of 1.0 M CH3NH3+Cl-? (Kb for CH3NH2 is: 5.2 x 10-4 ) I’m having a hard time figuring out what to do first. is the ICE table come in handy

asked by Maria on January 18, 2015
CHEM
Calculate the equilibrium constant for the weak base CH3NH2, if a solution of the base with an initial concentration of 7.05×10-4 M has a [CH3NH3+] of 0.000379 M (make an exact calculation assuming that initial concentration is not equal to the

asked by harry on April 26, 2009
chemistry 1046
Solve an equilibrium problem (using an ICE table) to calculate the pH of each solution. a solution that is 0.266 M in CH3NH2 and 0.134 M in CH3NH3Br. Kb = 4.4e-4

asked by Anonymous on July 3, 2012
Chemistry
What is the pH of a buffer solution that is 0.20M methylamine and 0.15 M methylammonium chloride. which do i get the pH of

asked by LT on April 2, 2008
Chemistry Kb question need to clarify something
the pKb for methylamine is 3.36, what is the Kb for methylamine? pKa+pKb= 14.00 Kb= 10^-pKb = 4.4×10^-4 is the answer but HOW?? what is punched into the calculator to get 4.4 x 10^-4??

asked by Lori on December 16, 2010
Chemistry II
Calculate the pH at the equivalence point in the titration of 50ml of 0.20 M methylamine (Kb=4.3*10^-4) with a 0.40 M HCL solution.

asked by Katie on May 3, 2013
Chemistry
How many moles of HCl must be added to 100mL of a 0.100 M solution of methylamine (pKb=3.36) to give a buffer having a pH of 10.0?

asked by Joe on April 24, 2011
Chemistry
What is the kb of a 0.0200 m ( at equilibrium) solution of methyl amine, ch3nh2, that has a ph of 11.40?

asked by Dylan on July 2, 2016
Chemistry
Calculate pH of a solution that is 0.255M in CH3NH2 and 0.105M in CH3NH3Br

asked by Gabby on March 6, 2015
Chemistry
What is the pH of a 0.77M solution of methylamin at 25 degree C? CH3NH2, Kb= 4.4X10-4? How do I set this up to get the answer?

asked by George on March 7, 2013

Chemistry
What is the pH at the equivalence point for the titration of 0.26M CH3NH2(aq) with 0.26M HClO4(aq)? For CH3NH2, Kb = 3.6 x 10^-4. I arrived to the answer of pH=5.57 but its wrong. Can you tell me why it is wrong? Thanks!

asked by Ron A. on June 5, 2010
chemistry
One has a solution Sa of ethanoic acid of concentration Ca=1×10^-2 mol/l and pH=3.4 One mixes a volume Va=60ml of the solution Sa of ethanoic acid with a volume Vb1=20ml of the Sb1 solution of ammonia of concentration Cb1=2×10^-2 mol/l. The pH is 5 One

asked by vicky on December 25, 2016
chemistry
One has a solution Sa of ethanoic acid of concentration Ca=1×10^-2 mol/l and pH=3.4 One mixes a volume Va=60ml of the solution Sa of ethanoic acid with a volume Vb1=20ml of the Sb1 solution of ammonia of concentration Cb1=2×10^-2 mol/l. The pH is 5 One

asked by vicky on December 27, 2016
Chemistry
Hello, i seem to be stuck on a problem and do’nt know why im not gettin the right answer.I have the he Ka and Kb values for each of the weak acids and bases from the chart and I keep getting zero and the second one 2.27*10^-24 is this correct?? Thank uu

asked by Amy Wight on March 24, 2011
Chemistry
Hello, i seem to be stuck on a problem and do’nt know why im not gettin the right answer.I have the he Ka and Kb values for each of the weak acids and bases from the chart and I keep getting zero and the second one 2.27*10^-24 is this correct?? Thank uu

asked by Amy Wight on March 24, 2011
Chemistry
Hello, i seem to be stuck on a problem and do’nt know why im not gettin the right answer.I have the he Ka and Kb values for each of the weak acids and bases from the chart and I keep getting zero and the second one 2.27*10^-24 is this correct?? Thank uu

asked by Amy Wight on March 24, 2011
AP Chemistry
Which solution has the highest pH? 1. 0.1 M C6H5NH3Cl, Kb C6H5NH2 = 4.2 × 10−10 2. 0.1 M NH2(OH)2Cl, Kb NH2OH = 6.6 × 10−9 3. 0.1 M NaCl, Kb  zero 4. 0.1 M NH4Cl, Kb NH3 = 1.8 × 10−5 5. 0.1 M CH3NH3Cl, Kb CH3NH2 = 5.0 × 10−4

asked by Anonymous on February 25, 2014
Chemistry
In a 1.0× 10–2 M solution of CH3NH3Br(aq), identify the relative molar amounts of these species. H2O, OH-, CH3NH3+, CH3NH2, H3O+, Br-, HBr

asked by Joe on March 28, 2016
science
Please help!! Methylamine has a vapor pressure of 344 torr at -25∘C and a boiling point of -6.4∘C . Find ΔHvap for methylamine. I know that ln(P1/P2)=(ΔHvap/R)(1/T2-1/T1) but it doesn’t indicate whether the boiling point is the “normal boiling

asked by caleigh on December 12, 2016
Chem
In a 1.0× 10–2 M solution of CH3NH3Br(aq), identify the relative molar amounts from highest to lowest for : -Br- -OH- -CH3NH3+ -HBr -CH3NH2 -H3O+ -H2O

asked by Rich on November 8, 2013

Chem- Bronsted bases
Which of the following substances can act as a Bronsted base in aqueous solution? (Select all that apply.) H2O NH3 H2 CH3NH2 O2 PH41+ CO32-

asked by Elizabeth on February 23, 2014
Chemistry
1) Which ion(s) below would undergo hydrolysis in water? A) Cl- B) K+ C) NH4+ D) NO3- E) Two of the above My guess is C, but I’m not too sure about this one. 2) Calculate the [OH-] present in solution labeled 1.73 M methylamine. CH3NH3 + H2O –> CH3NH3+ +

asked by Amanda on May 1, 2014
Science
What concentration of CH3NH3Br is necessary to prepare a pH = 10.00 buffer solution assuming the base concentration is 0.49 M (Kb for CH3NH2 = 4.4 x 10-4).

asked by Yanis on May 1, 2013
Chem
What concentration of CH3NH3Br is necessary to prepare a pH = 10.00 buffer solution assuming the base concentration is 0.49 M (Kb for CH3NH2 = 4.4 x 10-4). In M

asked by Yanis on May 1, 2013
chemistry!
a) Find the pH at the equivalence point when 40ml of 0.025 M of methylamine (NH2CH3 and Kb = 4.4×10^-4) is titrated with 0.025 M HCl. b) The Kf for the complex ion Ag(NH3)2+ is 1.7×10^7. The Ksp for AgI is 1.5×10^-16. What is the molar solubility of AgI in

asked by Freddy on November 17, 2015
Science
Determine the pkb of methylamine if the kb is 4.4*10^-4.

asked by Terry on March 16, 2014
chemistry
What is the chemical equation of methylamine with CuSO4?

asked by Mikha on March 21, 2013
chemistry
What is the net ionic equation for the reaction of formic acid and methylamine

asked by lora on March 17, 2019
College Chemistry
Calculate the pH at the equivalence point in the titration of 55.0 mL of 0.180 M methylamine(Kb = 4.4 × 10−4) with 0.330 M HCl.

asked by Emily on March 29, 2017
Chemistry
what is the structure of CH3NH2 and CH3NH3

asked by Anonymous on February 28, 2011

CHEMISTRY- intermolecular forces
What intermolecular forces act in the following: H2 PH3 CH3NH2

asked by Jasmin on November 3, 2010
Chemistry
Suppose that 50.0 mL of 0.25 M CH3NH2(aq) is titrated with 0.35 M HCl(aq). (a) What is the initial pH of the 0.25 M CH3NH2(aq)? (b) What is the pH after the addition of 15.0 mL of 0.35 M HCl(aq)? (c) What volume of 0.35 M HCl(aq) is required to reach

asked by Dana on November 3, 2010
Chemistry
what mass of water will be formed by reaction of 3.50g of methylamine (8CH3NH2) with 15.0g of perchloric acid (13HClO4)? Answer is 99.1. How do you work this?

asked by Michelle on November 6, 2012
Chem
Methylaime, CH3NH2. If a 0.100 mol/L solution of methyamine has a pH of 11.80, calculate the ionization constant for the weak base. What is an ionization constant. Is it just K? This is what I did so far: 11.80 = -log (concentration of h3o+) 10^-11.80 =

asked by Lena on July 23, 2009
Chemistry
State whether each of the following aqueous solutions would be acidic, basic, or neutral. Include appropriate net-ionic equations to show why a given solution is acidic or basic. a) NaNO3 b)KC6H5CO2 c)50:50 mixture of C6H5CO2H+KC6H5CO2 d)(CH3NH3)Cl e)50:50

asked by Anonymous on March 12, 2010
college chemistry
Which base listed below would be the best to creat a buffer having a pH of 5.0230? hydrazine, Kb = 8.90e-7 methylamine, Kb = 3.70e-4 ethanolamine, Kb = 3.20e-5 pyridine, Kb = 1.40e-9

asked by hershi on April 5, 2014
Relative Acidities
Rank the given compounds on their relative acidity. Here was the order I thought it was but it turned out to be wrong. (i based it based off of sp being most acidic and sp3 being least acidic) STRONGEST HC(triple bond)C-CH3 H2C=CH2 CH3NH2 H2O CH4–>

asked by Allie on February 16, 2011
chemistry
Out of the following compounds, which one is the weakest base? NH3, CH3NH2, NH2F, NH2Br

asked by Anonymous on July 19, 2010
chem
a soln. that is .195 M in CH3NH2 and .105 M in CH3NH3Br what is the balanced equation for this ? How do you know ?

asked by natash on March 8, 2009
AP Chemistry
In the titration of 50.0 mL of 1.0 M CH3NH2 (kb=4.4 x 10^-4), with 0.50 M HCl, calculate the pH a) after 50.0 mL of 0.50 M has been added b) at the stoichiometric point.

asked by some kid on March 29, 2009

chemistry
how do you identify the base in this reaction? h2o(L) + CH3NH2(aq) yields OH-(aq) + CH3+(aq)

asked by ryan on May 12, 2012
chemistry
what is the formula of the product form when CH3NH2 reacts eith hydrogen ion?

asked by mano on October 9, 2010
Chemistry
what mass of nitrogen dioxide (8NO2) will form by reaction of 3.50 mole of perchloric acid (13HClO4) with excess methylamine (8CH3NH2)? Answer is 99.1 g. How do you work this?

asked by Michelle on November 6, 2012
Chemistry
State whether each of the following aqueous solutions would be acidic, basic, or neutral. Include appropriate net-ionic equations to show why a given solution is acidic or basic. a) NaNO3 b)KC6H5CO2 c)50:50 mixture of C6H5CO2H+KC6H5CO2 d)(CH3NH3)Cl e)50:50

asked by Julie on March 13, 2010
Chemistry
Complete and balance the following (CH3)2NH(aq)+CH3COOH(aq)→ CH3CH2NH2(aq)+HBr(aq)→ CH3NH2(aq)+HCOOH(aq)→

asked by Nancy on May 27, 2014
Chemistry
Consider the titration: .30 M HCl versus .30 M methlamine (CH3NH2). What is the concentration of CH3NH3+ at the equivalence point?

asked by Amy on November 29, 2010
chem
I am trying to figure out how to calculate the ratio of CH3NH2 to CH3NH3Cl required to create a buffer with pH of 10.26, I’m not sure where to start.

asked by moe on October 25, 2010
chem
I am trying to figure out how to calculate the ratio of CH3NH2 to CH3NH3Cl required to create a buffer with pH of 10.26, I’m not sure where to start.

asked by moe on October 25, 2010
Chemistry
Calculate the pH at the equivalence point for the titration of 0.120 M methylamine with 0.120 M HCl (kb of methyalamine is 5.0 x 10^-4)

asked by Mariana on November 13, 2011
Chemistry
Complete and balance the reactions A) (CH3)2NH(aq)+CH3COOH(aq)→ B) CH3CH2NH2(aq)+HBr(aq)→ C) CH3NH2(aq)+HCOOH(aq)→

asked by Tim on June 3, 2014

Chem
Complete and balance the reaction of A) (CH3)2NH(aq)+CH3COOH(aq)→ B) CH3CH2NH2(aq)+HBr(aq)→ C) CH3NH2(aq)+HCOOH(aq)→

asked by Alex on June 2, 2014
chemistry
What volume of titrant would be required to reach the equivalence point in the titration of 25.0 mL and 0.825M CH3NH2 with 1.00 M HCL?

asked by Anonymous on October 19, 2011
Chemistry!!
Complete and balance the reaction of A) (CH3)2NH(aq)+CH3COOH(aq)→ B) CH3CH2NH2(aq)+HBr(aq)→ C) CH3NH2(aq)+HCOOH(aq)→

asked by Alex on June 2, 2014
chem
Arrange the following amines in order of decreasing base strength. NH3, NH2Br, CH3NH2, (CH3)2NH

asked by help!!! on February 16, 2009
science

1. Which of the following is TRUE regarding this situation: Solution A has a pH of 7.38, and Solution B has a pH of 7.42? a.Solution B is more acidic than Solution A b.The pH of Solution A falls within the homeostatic pH range for extracellular body

asked by a on January 28, 2013