We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
For this question, we have a 17 ml solution of 1.7M ammonia, Kb=1.8x105 a) What is...
For this question, we have a 17 mL solution of 1.7M ammonia, Kb=1.8x10-5 a) What is the initial pH? b) What is the pH when 40 mL of 0.17 M HCl has been added? c) Where was the equivalence point volume? d) What is the pH when 8 mL of HCl has been added?
A solution of 0.0480 M HCl is used to titrate 27.0 mL of an ammonia solution of unknown concentration. The equivalence point is reached when 15.5 mL HCl solution have been added. (Assume Kw = 1.01× 10-14.) (a) What was the original pH of the ammonia solution? 匹の10.85 (b) What is the pH at the equivalence point? の5.50 (c) Draw a titration curve for this titration. ( r curve should be quantitative; calculate the pH at different points to construct...
You have 15.00 mL of a 0.100 M aqueous solution of the weak base C5H5N (Kb = 1.50 x 10-9). This solution will be titrated with 0.100 M HCl. (a) How many mL of acid must be added to reach the equivalence point? (b) What is the pH of the solution before any acid is added? (c) What is the pH of the solution after 10.00 mL of acid has been added? (d) What is the pH of the solution...
You have 25.00 mL of a 0.100 M aqueous solution of the weak base CH3NH2 (Kb = 5.00 x 10-4). This solution will be titrated with 0.100 M HCl. (a) How many mL of acid must be added to reach the equivalence point? (b) What is the pH of the solution before any acid is added? (c) What is the pH of the solution after 5.00 mL of acid has been added? (d) What is the pH of the solution...
You have 40.00 mL of a 0.300 M aqueous solution of the weak base C6H5NH2 (Kb = 4.00 x 10-10). This solution will be titrated with 0.300 M HCl. (a) How many mL of acid must be added to reach the equivalence point? (b) What is the pH of the solution before any acid is added? (c) What is the pH of the solution after 10.00 mL of acid has been added? (d) What is the pH of the solution...
A solution of 0.0470 M HCl is used to titrate 29.0 mL of an ammonia solution of unknown concentration. The equivalence point is reached when 15.5 mL HCl solution have been added. (Assume Kw = 1.01 ✕ 10−14.) (a) What was the original pH of the ammonia solution? WebAssign will check your answer for the correct number of significant figures (b) What is the pH at the equivalence point?
Calculate the pH for 100. mL of a 0.500 M solution of ammonia, (NH3 Kb=1.8x10-5) being titrated with 0.500 M HCl at the following positions in the titration. i) The initial pH (before any HCl has been added). A. 9.44 B. 10.81 C. 11.48 D. 12.00 E. 11.75
need help calculating 100% and 105% please!
Kb of Ammonia = 1.8 x 10^-5
Thank you
pH Titration Curve A 40.0 mL sample of a 0.30 M solution of NH, is titrated with a 0.50 M HCl solution. Calculate the pH of the solution when the following percentages of the HCl solution required to reach the equivalence point have been added. Plot the data you determined for the pH at various points in the titration. o What is the pH...
Your job is to determine the concentration of ammonia in a commercial window cleaner. In the titration of a 25.0 mL sample of the cleaner, the equivalence point is reached after 11.0 mL of 0.175 M HCl has been added. What is the initial concentration of ammonia in the solution? What is the pH of the solution at the equivalence point?
Your job is to determine the concentration of ammonia in a commercial window cleaner. In the titration of a 25.0 mL sample of the cleaner, the equivalence point is reached after 13.3 mL of 0.141 M HCl has been added. What is the initial concentration of ammonia in the solution? What is the pH of the solution at the equivalence point?