A 250.0 mL solution of a strong acid is found to have a pH of 0.54. What is the labeled (initial) concentration of this acid?
pH = 0.54
[H+] = 10^(-pH) = 10^(-0.54) = 0.2884 M
So,
[H+] = [Acid] = 0.2884 M
Total moles = 0.2884 * 0.250 = 0.0721 moles
250 ml contains = 0.0721 moles
So, 1000 ml will contain = 0.0721 * 1000/250 = 0.2884 moles
Hence, strong acid concentration = 0.29 M
A 250.0 mL solution of a strong acid is found to have a pH of 0.54....
A chemist must prepare 250.0 ml of hydrochloric acid solution with a pH of 1.80 at 25°C. He will do this in three steps: Fila 250.0 ml. volumetric flask about halfway with distilled water. • Measure out a small volume of concentrated (6.0 M) stock hydrochloric acid solution and add it to the flask. . Fill the flask to the mark with distilled water, Calculate the volume of concentrated hydrochloric acid that the chemist must measure out in the second...
Calculate the ph of a solution prepared by mixing 2.0 mL of a strong acid solution of pH 3.00 and 3.0 mL of a strong base of pH 10.00.
2)250.0 mL of a 0.375 M solution of lactic acid (HC:H:03) is titrated with a solution of 0.75 M NaOH. The K, for lactic acid is 1.38 x 104. (22 pts total) a) what is the pH before addition of NaOH? (Hint: what is the relevant equilibrium?) (4 pts) b) what is the total number of moles of acid? (2 pts) c) what volume of the NaOH solution is required to reach the equivalence point? (2 pts) d) what is...
2. A Student wants to prepare 250.0 mL of pH 4.1 buffer solution. He is planning to use formic acid (HCOOH) and sodium formate (HCOONa) for this job. What should the mass of sodium formate that he should add to 250,0 mL of 0.20 M formic acid solution to prepare this buffer? (K =1.8x10 for formic acid.) 3. If 0.10 M solution of a weak acid has a pH of 3.90, find the Ka for the acid.
Calculate the pH of a strong acid solution formed by mixing 83.3 mL of 0.0297 M HBrO4 with 77.2 mL of 0.129 M HNO3. a) The pH of this solution is 0.8. b) The pH of this solution is 1.1. c) The pH of this solution is 0.5. d) The pH of this solution is 4.4. e) The pH of this solution is 1.9.
An acid-base titration is performed: 250.0 mL of an unknown concentration of HCl(aq) is titrated to the equivalence point with 36.7 mL of a 0.1000 M aqueous solution of NaOH. Which of the following statements is not true of this titration? A. At the equivalence point, the OH−concentration in the solution is 3.67×10−3 M. B. The pH is less than 7 after adding 25 mL of NaOH solution. C. The pH at the equivalence point is 7.00. D. The HCl...
what is the ph of a solution of a strong acid with a concentration .007 M
Titration of a diprotic acid with a strong base You have a 10.0 mL solution containing 0.5 M carbonic acid. Carbonic acid is diprotic, with pKa1 = 6.35 and pKa2 = 10.33. You titrate this solution using 1.00 M NaOH . (a) Calculate the pH of the solution before adding any NaOH. (b) Calculate the amount of NaOH needed to reach the first midpoint. What is the pH? (c) Calculate the amount of NaOH needed to reach the first equivalence...
4. (5 pts) A pH of solution of a weak acid is 2.0. If 100.0 mL of this solution is diluted to 400 mL, then the pH of new solution will be..... Explain your answer. Assume that initial concentration of weak acid is much larger than the concentration of hydronium ions.
Explain why a weak acid solution has a higher pH than a strong acid solution concentration. of the same Explain why the equivalence point of a weak acid titrated with a strong base occurs at a basic pH.