Analytical Chemistry

Analytical chemistry
1. What is the [OH–] if the [H3O+] is 6.12 ´ 10–5 M?
2. Predict the pH and composition of a solution prepared by adding 0.090 mol of HF to 0.040 mol Using the ladder diagram in Figure 6.7, predict the result of adding 0.080 mol
3. of Ca2+ to 0.060 mol of Mg (EDTA)2–. EDTA is an abbreviation for the ligand ethylenediaminetetraacetic acid. Of NH3
4. Calculate the pH of 0.050 M NH3. State any assumptions made in simplifying the calculation, and verify that the error is less than 5%.
5. Calculate the pH of 0.10 M Na2HPO4.
6. Calculate the pH of a buffer that is 0.020 M in NH3 and 0.030 M in NH4Cl. What is the pH after adding 1.00 mL of 0.10 M NaOH to 0.10 L of this buffer?
7. 7. Using the systematic approach, calculate the pH of the following solutions
a. 0.050 M HClO4
b. 1.00 ´ 10–7 M HCl
c. 0.025 M HClO
d. 0.010 M HCOOH
e. 0.050 M Ba(OH)2
f. 0.010 M C5H5N
8. Calculate the pH of the following acid–base buffers
a. 100 mL of 0.025 M formic acid and 0.015 M sodium formate b. 50.00 mL of 0.12 M NH3 and 3.50 mL of 1.0 M HCl
c. 5.00 g of Na2CO3 and 5.00 g of NaHCO3 in 0.100 L
9. Calculate the pH of the buffers in problem 19 after adding
5.0 ´ 10–4 mol of HCl.
10. Calculate the pH of the buffers in problem 19 after adding
5.0 ´ 10–4 mol of NaOH
11. Calculate pH of buffer solution, prepared of 30 ml of 0,1n acetic acid solution and 10 ml of 0,ln sodium acetate solution: