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Brainly.com What is your question? High School Mathematics 5+3 pts Which of the following situations could be represented with the given system of equations? 0.1x+0.6y=0.4(5) x+y=5 A. Eunice needs to combine solutions of 0.1M HCl and 0.4M HCl to produce 5L of 0.6M hydrochloric acid (HCl). B. Eunice needs to combine solutions of 0.1M HCl and 0.6M HCl to produce 5L of 0.4M hydrochloric acid (HCl). C. Eunice needs to combine solutions of 0.4M HCl and 0.6M HCl to produce 5L of 0.1M hydrochloric acid (HCl). D. Eunice needs to combine solutions of 0.1M HCl and 0.6M HCl to produce 4L of 0.5M hydrochloric acid (HCl).

Answered by answersmine AT 22/10/2019 – 02:26 AM In the equations, the molarity is given as coefficients, x and y are volumes of HCl of different concentrations.  Therefore on the right hand side, molarity is 0.4, volume is 5 L.The correct answer has a product of 0.4M and 5L.

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A 150ml sample of hydrochloric acid completely reacted with 60.0mL of a 0.100 M NaOH solution. What was the original concentration of the HCl solution

A 150ml sample of hydrochloric acid completely reacted with 60.0mL of a 0.100 M NaOH solution. What was the original concentration of the HCl solution

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What volume 12.6 M HCL must be added to enough water to prepare 5.00 litters of 3.00 M HCL?

To solve this problem, we shall use the role;M1V1 = M2V2M1: is the molarity of the solution before dilution.V1: is the volume of the solution that we need to dilute.M2: is the molarity of the solution after dilution.V2: is the volume of the solution after dilution. By substitution;12*V1 = 3*5V1 …

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A second reaction mixture was made up in the following way: 10 mL 4.0 M acetone + 20 mL 1.0 M HCl + 10 mL 0.0050 M I2 + 10 mL H2O a. What were the initial concentrations of acetone, H+ ion, and I2 in the reaction mixture? (acetone) ___________ M; (H+) ___________ M; (I2)0 ___________ M b. It took 120 seconds for the I2 color to disappear from the reaction mixture when it occurred at the same temperature as the reaction in Problem 2. What was the rate of the reaction?

A. We can calculate the initial concentrations of each by the formula: initial concentration ci = initial volume * initial concentration / total mixture volume where, total mixture volume = 10 mL + 20 mL + 10 mL + 10 mL = 50 mL ci (acetone) = 10 mL * …

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A second reaction mixture was made up in the following way: 10 mL 4.0 M acetone + 20 mL 1.0 M HCl + 10 mL 0.0050 M I2 + 10 mL H2O a. What were the initial concentrations of acetone, H+ ion, and I2 in the reaction mixture? (acetone) ___________ M; (H+) ___________ M; (I2)0 ___________ M b. It took 120 seconds for the I2 color to disappear from the reaction mixture when it occurred at the same temperature as the reaction in Problem 2. What was the rate of the reaction?

A. We can calculate the initial concentrations of each by the formula: initial concentration ci = initial volume * initial concentration / total mixture volume where, total mixture volume = 10 mL + 20 mL + 10 mL + 10 mL = 50 mL ci (acetone) = 10 mL * …

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When hydrochloric acid reacts with sodium sulfide, hydrogen sulfide gas and sodium chloride are produced. How many moles of H2S will be generated by 2.56 moles of HCl? 2HCl + Na2S → H2S + 2NaCl A 10 liters B 0.1 liters C 40 liters D 20 liters

When hydrochloric acid reacts with sodium sulfide, hydrogen sulfide gas and sodium chloride are produced. How many moles of H2S will be generated by 2.56 moles of HCl? 2HCl + Na2S → H2S + 2NaCl A 10 liters B 0.1 liters C 40 liters D 20 liters

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How would you prepare 10 ml of a 0.25% m/v hcl solution if 1% m/v hcl was available? how much 1% m/v hcl is needed? how much distilled water is used?

This problem is to apply Roult’s Law. Roult’s Law states that the vapor pressure, p, of a solution of a non-volatile solute is equal to the vapor pressure of the pure solvent, Po solv, times the mole fraction of the solvent, Xsolv p = Xsolv * Po sol X solv …

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Which element(s) is being reduced in the redox reaction below? 6 nh4clo4 (s) + 10 al(s) 5 al2o3 (g) + 6 hcl (g) + 3 n2 (g) + 9 h2o (g) n and al h cl o?

Which element(s) is being reduced in the redox reaction below? 6 nh4clo4 (s) + 10 al(s) 5 al2o3 (g) + 6 hcl (g) + 3 n2 (g) + 9 h2o (g) n and al h cl o?

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In the covalent bond between hydrogen and chlorine in the HCl molecule, where will the majority of shared electrons be found? A.near the hydrogen atom B.near the chlorine atom C.equidistant from both atoms D.away from chlorine atom E.away from both atoms

When ammonia is added with water, it forms a lonely OH- ion and a conjugate acid of HNH3+, or NH4+. Just based on the formula alone, a basic hydroxide is one of the products from NH3 and H2O, which is usually a tall-tale sign of NH3 being basic. Also, the …

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Aqueous magnesium chloride and hydrogen gas are produced when solid magnesium reacts with aqueous hydrochloric acid (HCl). What is the equation for this reaction? Do not worry about balancing this equation.

Explanation : In the net ionic equations, we are not include the spectator ions in the equations. Spectator ions : The ions present on reactant and product side which do not participate in a reactions. The same ions present on both the sides. (a) The given balanced ionic equation is, …

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In the reaction Na2CO3 + 2HCl → 2NaCl + CO2 + H2O, how many grams of CO2 are produced when 7.5 moles of HCl is fully reacted?

Answer: The coefficient of CO₂ is 5. Explanation:     Balancing the reaction: ___C₅H₁₂ + ___O₂ → ___CO₂ + ___H₂O There are 5 C in the left side, so we put 5 on the right side: ___C₅H₁₂ + ___O₂ →  5CO₂ + ___H₂O There are 12 H in the left …

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Consider the reaction. mc028-1.jpg Which statement is true at STP? (The atomic mass of Zn is 65.39 u.) 2 mol of HCl produce 1 L of H2 gas. 1 L of Zn produces 1L of H2 gas. 65.39 g of Zn produce 22.4 L of H2 gas. 1 L of HCl produces 1 mol of H2 gas.

Consider the reaction. mc028-1.jpg Which statement is true at STP? (The atomic mass of Zn is 65.39 u.) 2 mol of HCl produce 1 L of H2 gas. 1 L of Zn produces 1L of H2 gas. 65.39 g of Zn produce 22.4 L of H2 gas. 1 L of …

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By titration it is found that 68.5 ml of 0.154 m naoh(aq) is needed to neutralize 25.0 ml of hcl(aq). calculate the concentration of the hcl solution.

Answer: The mass of sodium sulfide needed is 195000 mg. Explanation: To calculate the moles of cadmium nitrate, we use the equation: Molarity of cadmium nitrate = 0.0100 M Volume of cadmium nitrate = 25.0 mL = 0.025 L   (Conversion factor: 1 L = 1000 mL) Putting values in …

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Which combination will make a buffer? NaOH and NaCl KOH and KCl HCl and NaCl CH3COOH and CH3COONa

Answer: 0.5 M ionic Explanation: Addition of nonvolatile solute depresses the freezing point of a solvent. As depression in freezing point is a colligative property, which means it depends on the amount of solute. Thus more is the no of ions, more is the depression in freezing point. =Depression in …

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What is the concentration of a solution prepared by adding 50.0 mL of a 3.0 M HCl solution to a 250 mL volumetric flask and filling to the mark with water?

Explanation: a) Mass of potassium sulfate = 177 mg =0.177 g 1 g= 1000 mg Molecular mass of potassium sulfate = 174.24 g/mol Moles of potassium sulfate,n = b) 1 mol = 1000 milli moles 0.001016  mol =0.001016 × 1000 milli moles = 1.016 milli moles c) n = moles …

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