Vhat is the pH of a buffer that consists of 0.20 M NaH,PO4 and 0.40 M Na,HPO4? Ka1 = 7.5x 103 Ka2 = 6.2 x 108 Ka2 = 4.2 x 10-13 Express vour answer in decimal notation rounded to three significant figures.

What is the function of indicator in a titration? Edit View Insert Format Tools Table 12pt ✓ Paragraph BIU IU AT²V 2 T² : C

A 39.0 mL sample of a 0.540 M aqueous hypochlorous acid solution is titrated with a 0.390 M aqueous solution of sodium hydroxide. How many milliliters of sodium hydroxide must be added to reach a pH of 7.176? mL

pH: 3 [H*]: 10-3 M [OH]: 10-11 M 14 1 1 7 · 10-7 10-7 10-14 10-14 Dip litmus paper into the solution or add a drop of universal indicator. Use the sliders to change the pH of the solution and observe the effect on the indicators. Click Reset to start over. Help Reset The solution turns orange when the univeral indicator is added to it. Is the solution basic, acidic, or neutral?

You have 1.5 liter of solution that is composed of 8.88 grams of NH3 and 11.33 grams of ammonium chloride mixed well. Kb for ammonia =1.8 x 10^-5 (A) is this a buffer solution? Why or why not? (B)if it is a buffer solution, what is the pH of this buffer solution? (C)how many mL of 1.50 M HCl can be added to this solution before the buffer is exhausted (d) how many mL of 1.5 M NaOH can be added to this solution before the buffer is exhausted?

please answer both for a vote uofront. thanks (Please type answer no write by hend)

Consider the “window cleaner” problem, question 2 on page 12 of your lecture notes. Suppose that prior to the titration, the 10 mL sample of window cleaner was diluted by adding about 10 mL of DI water so that the solution could have better contact with the pH meter. What effect would this dilution have on the volume of titrant needed? (a) The amount of titrant would be the same because the moles of analyte was not changed.(b) The amount of titrant would be doubled because the analyte solution volume was doubled.(c) The amount of titrant would be halved because the was diluted by half.

The Kb of hydroxylamine, NH2OH, is 1.10×10−8. A buffer solution is prepared by mixing 100.0 mL of a 0.99 M hydroxylamine solution with 50.0 mL of a 0.89 M HCl solution. Determine the pH of the resulting solution.

Equal volumes of the following pairs of solutions are mixed. Which pair will be a buffer solution? Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answe a b с d 0.10 M NH3 and 0.10 M NaOH 0.10 M HCl and 0.15 M KOH 0.10 M NaOH and 0.15 M HCN 0.10 M HBr and 0.20 M HBrO

Buffer solutions produce large changes in pH upon addition of small amounts of strong acid or strong base. Group of answer choices True False