Please help me solve If 50.0 mL of 0.250 M lactic acid is titrated with 20.0...
. 20.0 mL of 0.100 M lactic acid solution is titrated with 0.100 M NaOH solution. Calculate the pH of the contents of the Erlenmeyer flask at each of the following points during the titration. (a) When 0.00 mL of NaOH have been added. (2) (b) After 5.00 mL of NaOH have been added. (3) (c) After 20.0 mL of NaOH have been added. (3) (d) After 10.0 mL of NaOH have been added. (1) (e) After 25.0 mL of...
25. A 50.0 mL sample of 0.150 M weak acid was titrated with a 0,150 M NaOH solution. What is the pH after 30.0 mL of the sodium hydroxide solution is added? The Ka of the acid is 1.9x10(3 points) D) 4.78 E) None of these C) 3.03 (A) 4.90 B) 1.34 26. A 25.0 mL sample of 0.25 M hydrofluoric acid (HF) is titrated with a 0.25 M NaOH solution. What is the pH after 38.0 mL of base...
A 50.0 mL sample of 0.150 M sodium hydroxide is titrated with 0.250 M nitric acid. Calculate: a. the pH after adding 10.00 mL of HNO3 b. the pH after adding 40.00 mL of HNO3 c. the volume required to reach the equivalence point d. the pH at the equivalence point
*50
mL lactic acid*
1. Calculate the pH as 0.1000 M lactic acid is titrated with 0.1000 M NaOH at a. 0 mL NaOH b. 15.00 mL c. 25.00 mL d. 49.00 mL e. 50.00 mL f. 51.00 mL
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...
6. A student titrated 50.0 mL of the 0.10 M unknown diprotic H2A with 0. 10 M NAOH. After 25.0 mL of NaOH was added, the pH of the resulting solution was 6.70. After 50.0 mL of NaOH was added, the pH of the solution was 8.00. What are the values of Ka1 and Ka2?
6. A student titrated 50.0 mL of the 0.10 M unknown diprotic H2A with 0. 10 M NAOH. After 25.0 mL of NaOH was added,...
A 100.0 mL sample of 0.100 M NaOH is titrated with 0.250 M HNO3. Calculate the pH after addition of each of the following volumes of acid: (a) 0.0 mL (b) 20.0 mL (c) 40.0 mL (a) 60.0 mL
A 50.0 ml sample of 0.50 M acetic acid, ch3cooh is titrated with a 0.150 M NaOH solution. calculate the ph after 25.0 ml of the base have been added (ka=1.8x10^-5)
A 50.0 mL sample of 0.25 M formic acid (HCOOH) aqueous solution is titrated with 0.125 M NaOH solution. Ka of HCOOH = 1.7 x 10−4. a. Calculate the pH of the solution after 50 mL of NaOH solution has been added. b. How many mL of 0.125 M NaOH need to be added to the sample to reach the equivalence point? What is the pH at the equivalence point?
ASAP please
Consider the titration of 50.0 mL of 0.200 M hypochlorous acid HCIO (Ka = 3.5 x 10-8) with 0.250 M NaOH. 5- How many milliliters of NaOH are required to reach the equivalence point? a) b) Calculate the pH before titration c) Calculate the pH after adding 40.0 mL. of NaOH d) Calculate the pOH after adding 20.0 ml, of NaOH