Calculate the at the following points in the titration of 20.00 ml of 0.300 M CH...
2. Calculate the pH at the following point in the titration of 20.00 mL of0.500 M CH3COOH with 0.500 M NaOH. CH3COOH has a Ka = 1.8x10-5. (2.5 pts) a. pH before the addition of any NaOH. Include balanced chemical equation. b. pH after the addition of 8.00 mL of 0.500 M NaOH. Include balanced chemical equation. c. pH after the addition of 10.00 mL of 0.500 M NaOH. Include balanced chemical equation. d. pH after the addition of 20.00...
Find the pH during the titration of 20.00 mL of 0.2320 M nitrous acid, HNO2 (Ka = 7.1 ✕ 10-4), with 0.2320 M NaOH solution after the following additions of titrant. (a) 0 mL (b) 10.00 mL (c) 15.00 mL (d) 19.00 mL (e) 19.95 mL (f) 20.00 mL (g) 20.05 mL (h) 25.00 mL
Be sure to answer all parts. Find the pH during the titration of 20.00 mL of 0.2400 mol/L butanoic acid, CHCH2CH2COOH (Ka -1.54 x 10-5), with 0.2400 mol/L NaOH solution after each addition of titrant: (a) 0 mL (b) 10.00 ml. pH= (c) 15.00 mL d) 19.00 mLpH- (e) 19.95 mL (1) 20.00 mL (g) 20.05 mL pH= (h) 25.00 mL pH = pH = pH = pH = pH = Be sure to answer all parts. Find the pH...
Calculate the pH during the titration of 20.00 mL of 0.1000 M CH3COOH(aq) with 0.2000 M NaOH(aq) after 2.5 mL of the base have been added. Ka of acetic acid = 1.8 x 10-5. QUESTION 9 Calculate the pH during the titration of 30.00 mL of 0.1000 M ethylamine, C2H5NH2(aq), with 0.1000 M HCl(aq) after 26 mL of the acid have been added. Kb of ethylamine = 6.5 x 10-4. QUESTION 10 Calculate the pH during the titration of 20.00...
4. 25.0 mL sample of 0.10 M CH COOH is titrated with 0.12 M NaOH. Determine the pH of the solution a) Before the addition of the base. The Ka of CH COOH is 1.8 x 10-5. (10 points) b) After the addition of 15.0 mL of NaOH. The Ka of CH,COOH is 1.8 x 10-5. (10 points)
Find the pH during the titration of 20.00 mL of 0.1000 M butanoic acid, CH CH CH COOH (K, 1.54 x 10), with 0.1000 M NaOH solution after the following additions of titrant. (a) 11.00 mL: pH- (b) 20.40 mL: (c) 29.00 mL: pH =
what are the last three values? Be sure to answer all parts. Find the pH during the titration of 20.00 mL of 0.2400 mol/L butanoic acid, CHjCH2CH2COOH (Ka 1.54 x 10-5), with 0.2400 mo/L NaOH solution after each addition of titrant: (a) 0 mL (b) 10.00 ml. pH= 4.81 (c) 15.00 mL pH = 5.29 (d) 19.00 ml. pH = 6.08 (e) 19.95 mL pH = 7.41 (f) 20.00 mL pH= (g) 20.05 mLpH- (h) 25.00 mLpH- pH = 2.71...
Determine the pH during the titration of 29.5 mL of 0.324 M acetic acid (Ka = 1.8×10-5) by 0.414 M NaOH at the following points. (a) Before the addition of any NaOH ________ (b) After the addition of 5.70 mL of NaOH _______ (c) At the half-equivalence point (the titration midpoint) _______ (d) At the equivalence point _______ (e) After the addition of 34.6 mL of NaOH ________
20. Calculate the pH at the following points in the titration of 25.00 ml of 0.400 M HCIO with 0.400 M KOH. Ka=3.0x10 a. Before the addition of any KOH b. After the addition of 5.00 ml of 0.400 M KOH c. After the addition of 12.50 ml of 0.400 M KOH d. After the addition of 25.00 ml of 0.400 M KOH e. After the addition of 30.00 ml of 0.400 M KOH
8. Calculate the pH for the following cases in the titration of 25.00 mL of 0.200-M acetic acid, CH3COOH(aq), with 0.200 M NaOH(aq): (a) before addition of any NaOH(aq) (b) after addition of 5.00 mL of NaOH(aq) (c) after addition of 12.50 mL of NaOH(aq) (d) after addition of 25.00 mL of NaOH(aq) (e) after addition of 26.00 mL of NaOH(aq)