A solution of household bleach contains 5.25% sodium hypochlorite, NaOCI, by mass. Assuming that the density of bleach is the same as water, calculate the volume of household bleach that should be diluted with water to make 500.0 mL of a pH = 10.23 solution. Use the K₂ of hypochlorous acid found in the chempendix.

A solution of household bleach contains 5.25% sodium hypochlorite, NaOCI, by mass. Assuming that the density of bleach is the same as water, calculate the volume of household bleach that should be diluted with water to make 500.0 mL of a pH = 10.23 solution. Use the K₂ of hypochlorous acid found in the chempendix.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Please don't provide handwritten solution ....
A chemist must prepare 350.0 mL of hydrobromic acid solution with a pH of 1.80 at 25 °C. He will do this in three steps: • Fill a 350.0 mL volumetric flask about halfway with distilled water. • Measure out a small volume of concentrated (7.0M) stock hydrobromic acid solution and add it to the flask. • Fill the flask to the mark with distilled water. Calculate the volume of concentrated hydrobromic acid that the chemist must measure out in the second step. Round your answer to 2 significant digits. mL x10 Explanation Check O 2022 McGraw Hill LLC, All Rights Reserved. Terms of Use Privacy Center Acce: 80°F Cloudy DELL Esc F2 F3 F4 F5 F6 F7 F8 F9 F10 F11 F12 PrtScr Insert Delete F1 "R A # $4 & Backspace 1 3 4 6 80 E Y *00
A chemist must prepare 800.0 mL of potassium hydroxide solution with a pH of 12.30 at 25 °C. He will do this in three steps: ⚫ Fill a 800.0 mL volumetric flask about halfway with distilled water. • Weigh out a small amount of solid potassium hydroxide and add it to the flask. • Fill the flask to the mark with distilled water. Calculate the mass of potassium hydroxide that the chemist must weigh out in the second step. Round your answer to 2 significant digits.
▼ Part A Calculate the concentrations of NH and NH3 and the pH in a solution prepared by mixing 19.0 g of NaOH and 0.495 L of 1.5 M NH4Cl. Assume that the volume remains constant. Express your answers using two significant figures. Enter your answers numerically separated by a comma. 15. ΑΣΦ [NH ], [NH3] = Submit Part B PH = Submit Request Answer V—| ΑΣΦΑΛΟ Request Answer www. ? Seg ? M
1.) HA is a weak acid. Its ionization constant, Ka, is 3.1 x 10-13. Calculate the pH of an aqueous solution with an initial NaA concentration of 0.061 M. 2.) We place 0.149 mol of a weak acid, HA, in enough water to produce 1.00 L of solution. The final pH of the solution is 1.11 . Calculate the ionization contant, Ka, of HA. 3.)We place 0.527 mol of a weak acid, HA, and 12.0 g of NaOH in enough water to produce 1.00 L of solution. The final pH of this solution is 4.35 . Calculate the ionization constant, Ka, of HA.
7. Carbonic acid (H2CO3) is a diprotic acid with Ka1 = 4.30 × 10–7 and Ka2 = 5.60 × 10–11 What is the pH in a 1.834 M solution of carbonic acid? 8. The ionization constant, Kb, for weak base, B, is 7.56 × 10–5. What is the pH of a 0.6545 M solution of this base? The equation for the ionization of weak base B as follows. B (aq) + H2O(l) ⇌ BH+(aq) + OH⁻(aq)
1A) Calculate the concentration of C5H5N solution required to provide a pH of 9.29. The Kb of C5H5N is 1.7 × 10-9 at 25°C. 1B) Calculate the mass of C5H5N needed to prepare 2.20 L of the above solution. (Molar mass = 79.10 g/ mol) 2A) The acid-dissociation constant of hydrocyanic acid (HCN) at 25.0°C is 4.9 × 10-10, What is the pH of an aqueous solution of 0.80 M sodium cyanide (NaCN)? 2B) What would be pH of the above solution if NaCN was a strong base? 3A) Write the conjugate base of the following: a) C7H602. b) HCO3- c) ) HASO3²- 3B) Write the conjugate acid of the following: a) PH3 b) SiO32- c) BrO3" 3C) Using 3A-a (C7H6O2) and its conjugate-base as an example, prove that "KąKp = Kw" Search or type URL く=
A chemist dissolves 215. mg of pure sodium hydroxide in enough water to make up 190. mL of solution. Calculate the pH of the solution. (The temperature of the solution is 25 °C.) Round your answer to 3 significant decimal places. ☐ x10 G
A chemist must prepare 400.0 mL of hydrochloric acid solution with a pH of 1.20 at 25 °C. He will do this in three steps: • Fill a 400.0 mL volumetric flask about halfway with distilled water. • Measure out a small volume of concentrated (8.0M) stock hydrochloric acid solution and add it to the flask. • Fill the flask to the mark with distilled water. Calculate the volume of concentrated hydrochloric acid that the chemist must measure out in the second step. Round your answer to 2 significant digits. |mL x10
A chemist dissolves 891. mg of pure hydrochloric acid in enough water to make up 270. mL of solution. Calculate the pH of the solution. Round your answer to 3 significant decimal places. ☐ ☐ x10
A chemist must prepare 700.0 mL of sodium hydroxide solution with a pH of 12.30 at 25 °C. She will do this in three steps: • Fill a 700.0 mL volumetric flask about halfway with distilled water. • Weigh out a small amount of solid sodium hydroxide and add it to the flask. • Fill the flask to the mark with distilled water. Calculate the mass of sodium hydroxide that the chemist must weigh out in the second step. Round your answer to 2 significant digits. Ox10
A chemist dissolves 744. mg of pure hydrochloric acid in enough water to make up 250. mL of solution. Calculate the pH of the solution. Be sure your answer has the correct number of significant digits. 1.09 x10