20)
a)
pH = 1/2 (pKa - log C)
= 1/2 (4.74 - log 0.10)
pH = 2.87
b)
mmoles of NaOH = 1.5 x 0.1 = 0.15
mmoles of acid = 25 x 0.1 = 2.5
HA + NaOH -------------> A- + H2O
2.5 0.15 0 0
2.35 0 0.15
pH = pKa + log [A- / HA]
= 4.74 + log [0.15 / 2.35]
pH = 3.54
c)
volume of NaOH needed = 25 mL
d)
salt present = CH3COONa
sodium acetate salt present. this is basic .
e)
salt concentration = 25 x 0.1 / 50 = 0.05 M
pH = 7 + 1/2 (pKa + log C)
= 7 + 1/2 (4.74 + log 0.05)
pH = 8.72
f)
[H+] = 0.0167
pH = 1.78
20. a. Calculate the initial pH of a 0.10 M HAc solution. b. Calculate the pH...
Consider a titration of 250 mL 0.15 M acetic acid (Ka = 1.8 x10-5) with 0.10 M KOH. What is the pH of the acetic acid solution (ie: before the titration has begun?) What is the pH after adding 25 mL of 0.10 M KOH? What is the volume of base needed to reach the equivalence point? Is the pH at equivalence point acidic, basic, or exactly neutral? What is the pH after 500 mL of KOH has been added?
A titration is performed on 50mL of a 0.10 M solution of HN3 (Ka+1.9x10-5) with 0.10 M NaOH as the titrant. (a) What is the initial pH of the HN3 solution? (b) Calculate the pH of the solution after 25 ml of NaOH have been added (c) How many mL of NaOH are required to reach the equivalence point and what is the pH of the solution at the equivalence point.
10. Calculate pH of a solution formed by 20.0 mL of 0.10 M HNO, after 19.9 mL of 0.10 M KOH are added. 11. Which salt in water is acidic, basic, or neutral? AICI, NaBr, K,SOa, NH4I 12. The formula of a coordination compound is Li[Co(NHs)2(H2O)Clh . [26 pt) a) Name the coordination compound. b) Point out formulas of ligands. c) What is charge of Co? What is coordination number of the complex? d) Sketch all possible geometric isomers, labeling...
D Question 25 Calculate the pH of a 0.10 M CH3NH,Cl solution. Ky(CH NH) - 4.4x104 5.82 943 Сосоо 4.36 8.18 Question 26 5 pts When a strong acid is added to a strong base in a titration, what is expected at the equivalence point? A acidic solution from the conjugate acid of the strong base A neutral solution with a pH - 7 A acidic solution from the strong acid A basic solution from the strong base A basic...
1. 25.0 mL of a 0.100 M solution of NH, is titrated with 0.150M HCl. After 10.0 mL of the HCl has been added, the resultant solution is: A) Basic and before the equivalence point B) Basic and after the equivalence point C) Acidic and before the equivalence point D) Acidic and after the equivalence point E) Neutral and at the equivalence point
***A 50 mL solution of 0.10 M HC2H2O2 (aq) (K = 1.8 x 10-5) is titrated with 0.20 M NaOH (aq). " At the equivalence point is the solution acidic, basic, or neutral and why? o Basic because of excess OH O Basic because of hydrolysis of C2H302 o Neutral salt of strong acid and strong base O Basic because of hydrolysis of HC2H2O2 Acidic because of hydrolysis of Nat
Is the pH at the equivalence point in the titration of 0.10 M C2HSNH2 with 0.10 M HCI acidic, basic, or neutral? Explain your answer.
Learning Goal: To learn about titration types and how to calculate pH at different points of titration. In an acid-base titration, a titrant (solution of a base or acid) is added slowly to an analyte (solution of an acid or base). The titration is often monitored using a pH meter. A plot of pH as a function of the volume of titrant added is called a pH titration curve. Prior to the titration, the pH is determined by the concentration...
Assume that 28.0mL of a 0.10 M solution of a weak base B that accepts one proton is titrated with a 0.10 M solution of the monoprotic strong acid HA. A.) How many moles of HA have been added at the equivalence point? B.) What is the predominant form of B at the equivalence point? BA (aq), B(aq), BA-(aq), BOH-(aq), or BH+(aq)? C.) Is the pH more than, less than, or equal to 7 at the equivalence point? D.) Which...
1. For each of the following, predict whether an aqueous solution of the salt would be acidic, basic or neutral. Explain. a. Nacis b. NaF c. NHIS d. KHCO3 e. (CH3)2NH2NO31 2. What is the pH of a solution that is 0.060 M in potassium propionate (CH3CH2COOK) and 0.085M in propionic acid (CH3CH2COOH)? The Ka for propionic acid is 1.3x10-5.5 3. Suppose you need to prepare a buffer for a pH of 10.6. An acid-base pair (HA/A') to use has...