1. Calculate the pH: a) 0.005 n acetic acid solution; 2. What is the concentration of OH' ions in 0.05M NH,OH solution? What is the concentration of OH ions in 0.05M NH,OH solution containing an additional 0.1 mol / 1 NH,Cl? How many times does the presence of ammonium chloride in the solution lower concentration OH ions in the first solution? 3. Find out whether the precipitate is formed when mixing equal volumes of 0.001 n solutions of strontium chloride and potassium sulfate?

1. Calculate the pH: a) 0.005 n acetic acid solution; 2. What is the concentration of OH' ions in 0.05M NH,OH solution? What is the concentration of OH ions in 0.05M NH,OH solution containing an additional 0.1 mol / 1 NH,Cl? How many times does the presence of ammonium chloride in the solution lower concentration OH ions in the first solution? 3. Find out whether the precipitate is formed when mixing equal volumes of 0.001 n solutions of strontium chloride and potassium sulfate?

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter16: Acids And Bases

Section: Chapter Questions

Problem 7ALQ

See similar textbooks

Similar questions

The pH of a 0.20-M solution of HP is 1.92. Determine Ka far HF from these data.
. Which component of a buffered solution is capable of combining with an added strong acid? Using your example from Exercise 60, show how this component would react with added HC1.
A solution is made by dissolving 15.0 g sodium hydroxide in approximately 450 mL water. The solution becomes quite warm, but after it is allowed to return to room temperature, water is added to bring the volume to 500.0 mL of solution. (a) Calculate the pH and pOH in the final solution. (b) Why would we wait for it to return to room temperature? (c) If the mass of the water used to initially dissolve the sodium hydroxide were exactly 450 g and the temperature of the water increased by 8.865 C, how much heat was given off by the dissolution of 15.0 g of solute? Assume the specific heat of the solution is 4.184 J/g. K. What is the molar heat change for the dissolution of sodium hydroxide (known as the enthalpy of solution, Hsol)?
Which base in Table 14.3 is must appropriate for preparation of a buffer solution with a pH of 10.65? Explain your choice.
The pH of a 0.10 MHOBr solution is 4.8. What is H in that solution? ____________M What is OBr-? What is HOBr? Where do the H and OBr- ions comes from? ____________M; ____________M What is the value of Ka for HOBr? What is the value of pKa?____________ ____________
A student prepares 455 mL of a KOH solution, but neglects to write down the mass of KOH added. His TA suggests that he take the pH of the solution. The pH is 13.33. How many grams of KOH were added?
Consider a solution of an unknown salt having the general formula BHCl, where B is one of the weak bases in Table 13-3. A 0.10-M solution of the unknown salt has a pH of 5.82. What is the actual formula of the salt?
Consider an aqueous solution of HF. The molar heat of formation for aqueous HF is -320.1 kJ/mol. (a) What is the pH of a 0.100 M solution of HF at 100C? (b) Compare with the pH of a 0.100 M solution of HF at 25C.
Calculate the equilibrium concentration of the non-ionized acids and all ions in a solution that is 0.134 M in HNO2 and 0.120 M in HBrO.
How many grams of HI should be added to 265 mL of 0.215 M HCI so that the resulting solution has a pH of 0.38? Assume that the addition of HI does not change the volume of the resulting solution.