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77 solutions

Weak Base Strong Acid Titrations

Q. A 100 mL sample of 0.10 M HCl is mixed with 50 mL of 0.14 M NH3. What is the resulting pH? (Kb for NH3 = 1.8x10^-5) a. 12.30 b. 1.70 c. 3.04 d. 1.52 e. 10.96

Solved • Nov 4, 2019

Weak Base Strong Acid Titrations

Q. 100 mL of a buffer that consists of 0.20 M NH3 and 0.20 M NH4Cl is titratd iwth 25 mL of 0.20 M HCl. Calculate the pH of the resulting solution givent aht the Kb for NH3 is 1.8×10^-5. (A). 4.97 (B). 9.03 (C). 9,26 (D). 4.74 (E). 9.48

Solved • Nov 4, 2019

Weak Base Strong Acid Titrations

Q. 9. Find the pH of 60 mL of 0.8 M ammonia titrated with 100 mL of 0.6 M HCl. The Kb for ammonia is 1.8x10^-5

Solved • Oct 2, 2019

Weak Base Strong Acid Titrations

Q. An analytical chemist is titrating 184.6 mL of a 0.2300 M solution of trimethylamine ((CH3)3N) with a 0.1600 M solution of HNO3. The pKb of trimethylamine is 4.19. Calculate the ph of the base solution after the chemist has added 283.4 mL of the HNO3 solution to it. 2 decimal places for the answer

Solved • Oct 29, 2019

Weak Base Strong Acid Titrations

Q. An analytical chemist is titrating 222.7 mL of a 0.8000 M solution of dimethylamine ((CH3)2NH) with a 0.09200 M solution of HIO3. The pKb of dimethylamine is 3.27. Calculate the pH of the base solution after the chemist added 2100.2 mL of HIO3 solution to it. Round your answer to 2 decimal places.

Solved • Oct 29, 2019

Weak Base Strong Acid Titrations

Q. An analytical chemist is titrating 194.8 mL of a 1.800 M solution of ethylamine (C2H5NH2) with a 0.3600 M solution of HNO3. The pKb of ethylamine is 3.19. Calculate the pH of the base solution after the chemist has added 13.8 mL of the HNO3 solution to it. Round your answer to 2 decimal point places for final answer.

Solved • Oct 29, 2019

Weak Base Strong Acid Titrations

Q. A 22.9 mL sample of 0.309 M methylamine, CH3NH2, is titrated with 0.305 M perchloric acid. After adding 8.33 mL of perchloric acid, the pH is ___. Use the Tables link in the References for any equilibrium constants that are required.

Solved • Oct 26, 2019