Calculate the pH of the mixture when 200. mL of 0.20 M NaOH is mixed with 500. mL of 0.20 M HOCl. and equilibrium is reached. [Ka(HOCl) = 3.2 x 10 – 8]. Show the net ionic equations for any reactions that take place and the chemical reaction you are using to perform the pH calculation.
Calculate the pH of the mixture when 200. mL of 0.20 M NaOH is mixed with...
5 5 of the (original) mixture is titrated with 0.100 M NaOH. How many ml of this base c. 100.0 ml must be added to just reach a pH of 5.50 for the solution? Also determine d. Another 100.0 mL of the (original) mixture is mixed with 70.0 mL of 0.100 M NaOH. Determine the pH of the solution at this point. (Note that ascorbit acid is diprotic.) [H2Ab]-? o.Ou .o64 2. 400.0 mL of 0.100 M H2Ab (ascorbic a...
When 200 mL NaOH(aq) is added to 500 mL of 1.0 M HCL(aq), the pH of the resulting mixture is what?
27. Calculate the pH of a mixture made by adding 50.0 mL of 0.20 M HCI(aq) to 150.0 mL of water at 25.0°C A) 0.70 B) 1.00 C) 1.18 D) 1.30 E) 13.0 Ans: D 28. A mixture is made by adding 50.0 mL of 0.20 M NaOH(aq) to 50.0 mL of water. At 25.0°C, what is its pH? A) 1.00 B) 4.55 C) 7.00 D) 13.0 E) 13.3
Solve a, b and 2 1. Calculate the pH during the titration of 10.00 mL of 0.400 M hypochlorous acid with 0.500 M NaOH. First what is the initial pH (before any NaOH is added)? The Ka for HOCl is 3.0 x 10-8 M. Answer is 3.96 a. What is the pH after 10.60 mL of NaOH are added? b. What is the pH after 15.30 mL of NaOH are added? 2. Chloropropionic acid, ClCH2CH2COOH is a weak monoprotic acid...
3) Calculate the pH of the following solutions: a. 100.0 mL of 0.20 M HCH3CO2 (acetic acid), ka = 1.8x10 b. 100.0 mL of 0.20 M HCH,CO, plus 25.0 mL of 0.40 M NaOH c. 100.0 mL of 0.20 M HCH3CO, plus 50.0 mL of 0.40 M NaOH d. 100.0 mL of 0.20 M HCH,CO2 plus 75.0 mL of 0.40 M NaOH
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...
1)Calculate the pH during the titration of 10.00 mL of 0.400 M hypochlorous acid with 0.500 M NaOH. First what is the initial pH (before any NaOH is added)? The Ka for HOCl is 3.0 x 10-8 M. 2)How many mL of NaOH are added to reach the equivalence point 3) What is the pH after 2.40 mL of NaOH are added?
When 1.50 mL of 3.5-M Barium chloride is mixed with 2.50 mL of 0.65-M sodium sulfate, a precipitate forms. a. Write balanced chemical, ionic and net ionic equations for the reaction, including phase labels. b. Calculate the theoretical yield (in grams) of the precipitate and identify the limiting reactant. c.Calculate the grams of the reactant in excess (left over) after the reaction is complete.
Calculate the pH of a mixture of 51.0 mL of 0.106 M NaOH and 50.00 mL of 0.0950 M HNO3.
A 90.0-mL sample of 1.00 M NaOH is mixed with 45.0 mL of 1.00 M H_2SO_4 in a large Styrofoam coffee cup; the cup is fitted with a lid through which passes a calibrated thermometer. The temperature of each solution before mixing is 23.7degreeC. After adding the NaOH solution to the coffee cup and stirring the mixed solutions with the thermometer, the maximum temperature measured is 30.5degreeC. Assume that the density of the mixed solutions is 1.00 g/mL, that the...