Question

A. What is the ph of 10 ml of .10 M hcl, 5 ml of .10 M h2so4 and .060g of Naoh. Answer should be 1.70

B. What is the pH of a solution of ammonia 7% by weight (density 1.0g/ml). Answer should be 11.93

C. What is the pH or .30 M acetic acid with 41 g of sodium acetate per liter. Answer should be 5 grams

D. How many grams of the salt are required to prepare 100 ml of sodium acetate added to .10 M acetic acid to give ph of 6.00. Answer should be 14 grams

E. pH of .020 M ammonium sulfate. answer should be 5.32

F. pH of solution made by dissolving the following to give 100ml final solution

1.) .010 mole HNO2 and .0050 mol KNO2

2.) .010 mol HCl and .010 mol KNO2

3.) .010 mol KOh and .020 mol HNO2

Answer should be

1.) 2.99

2.) 2.15

3.) 3.29

I really have a hard time with the type of problems that you have to mix two things together. I never know how to set up the actual chemical equation, when to use ka/kb (and when not to), when to use the limiting reagent type step, and whether to multiply something my its stoichemteric coefficient. Are there any tips to remember these things ?