• example: Titration of 100.0 mL of 0.05 M NH3 with 0.10 M HCI • Calculate equivalence point volume • Calculate pH at the following volumes of acid added • 10.0 mL • 25.0 mL • 50.0 mL • 60.0 mL • Check your answers against the titration curve
3. Weak Base versus Strong Acid Derive a titration curve for the titration of 50.0 mL of 0.10 M NH3 (Kb=1.8 x 10-5) with 0.25 M HCl. Calculate the pH for the following volumes of HCl (0 mL, 10 mL, 15 mL, 20 ml, 25 mL, 30 mL, 35 mL). Volume of HCI, in milliters 0 pH (a) 10 15 (d) 20 |(f) 25 30 35 (g) pH at the equivalence point Specify your choice of indicator
4) Calculate the pH at the equivalence point for the titration below: 150 mL 0.10 M HCI against 75 mL of 0.20 M NH3
4) Calculate the pH at the equivalence point for the titration below: 150 mL 0.10 M HCI against 75 mL of 0.20 M NH3
10. For an aqueous solution labeled "0.10 M potassium bromide," A) the pH is greater than 7. B) the pH = 13. D) the pH is less than 7. E) the pH = 7. C) the pH = 1. 11. For a 0.10 M solution of a weak acid, HA, with pKa = 6, which of the following is true? A) [HA] =[A-] B) [HA] does not equal [H3O+] C) [HA] =[H3O] D) [HA] = K E) [HA] = 0...
7. In the titration of 10.0 mL of 0.500 M NH3 with 0.5 M HCI, calculate the pH of the following and sketch the titration curve. Kb 1.8 x 10 f. Before the titration starts g. After addition of 2.5 ml of HCl h. After addition of 5.0 ml of HCI i. After addition of 10.0 ml of HC
In the titration of 25.00 ml of 0.10 M HF with 0.10 M NaOHn given ka = 3.5 x 10-4 find initial PH, PH at the equivalence point and Ph at half equivalence point
What is the net ionic equation for the neutralization reaction between a HI with NH3? HI (aq) + NH3 (aq) ⇌ NH4I (aq), HI (aq) + OH- (aq) ⇌ H2O (l) + I- (aq), H3O+ (aq) + OH- (aq) ⇌ 2 H2O (l) H3O+ (aq) = NH3 (aq) = NH4+ (aq) + H2O (l) Which statement about buffers is NOT true? A buffer can be made by neutralizing some of the weak base in solution by adding a strong acid,...
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 student performs the titration of 25.0 mL of HCI with 0.1 M NaOH. If the acid concentration is 0.1 M and 35.0 mL of base are added, the hydroxide concentration and the pH are: [OH-] = 1.67 times 10^-2 M, pH = 12.22 [OH-] = 3.5 M, pH = 13.46 [OH-] = 1.67 times 10^-2 M, pH = 1.78 [OH-] = 2.58 times 10^-3 M, pH = 13.51 the pH at the equivalence point when a 0.20 M weak...
9.& 10.) A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Determine the pH of the solution at each addition of the HNO3. The Kb of NH3 is 1.8 x 10-5 (Yes, you may use the back or attach sheets to show your work.) Addition of HNO3 pH 150 200 Then sketch the titration curve for this titration. Make sure to label your axes (including numerically!), to indicate the equivalence point (and whether it is...