9. 15.00 mL of 0.100 M NaOH are added to 50.00 mL of a buffer solution containing 1.0 mmol CH3CO0H and 1.0 mmol CH3CO0. What is the new solution pH? (а) 11.89 (b) 2.11 (c) 7.87 (d) Can't tell / need more info.
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Mmoles of NaOH = molarity * volume ( in ml )
= 0.100 * 15.00
= 1.5 mmoles
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- If 8.5 g of solid NaC2H3O2 are dissolved in 100.0 mL of water, how many mL of 1.0 M HCl would need to be added to prepare a buffer solution that has pH of 4.60? (a) 40.0 mL (b) 48.0 mL (c) 60.0 mL (d) 75.0 mLA buffer is prepared by titrating a 100.0 mL sample of 0.10 M NH3 with 50.0 mL of 0.10 M HNO3. What is the pH of thebuffer?(a) 4.74(b) 7.78(c) 7.05(d) 9.2614) 40 ml of 0.0900 HCI is diluted to 100 ml with water and titrated with 0.1000M NAOH. Calculate the pH after the addition of the following volume (ml) of the titrant added: (a) 0.00 (b) 10.00 (c) 18.00 (d) 30.00 (e) 35.95 (f) 36.00 (g) 36.05 (h) 40.00
- Calculate the number of grams of ammonium chloride thatmust be added to 2.00 L of a 0.500 M ammonia solution to obtain a buffer of pH = 9.20. Assume the volume of thesolution does not change as the solid is added. Kb for ammoniais 1.80 x 10-5.(a) 60.7 g (b) 30.4 g (c) 1.52 g (d) 0.568 g(e) 1.59 x 10-5 g11. In which of the following solutions will HNO2 ionize less than it would in pure water? (a) 0.10 M NaCl (b) 0.10 M NaOH (c) 0.10 M KNO3 (d) 0.10 M NaNO2A 80.0 mL sample of 0.0200 M HCI is titrated with 0.0400 M KOH solution. Calculate the pH after the following volumes of base have been added. 6 19 (a) 17.2 mL (b) 39.2 mL (c) 40.0 mL pH= pH= pH = (d) 42.0 mL (e) 68.8 mL pH = pH = Hom Rece My s ook Ch 2: Us eacti Fe (2
- A 10.0-mL solution of 0.780 M NH, is titrated with a 0.260 M HCl solution. Calculate the pH after the following additions of the HCI solution: (а) 0.00 mL (b) 10.0 mL (с) 30.0 mL (d) 40.0 mLCalculate the pH change that results when 12 mL of 5.3 M NaOH is added to 768 mL of each the following solutions. (See the Acid-Base Table attached.) (a) pure water (b) 0.10 M NH4Cl (c) 0.10 M NH3(d) a solution that is 0.10 M in each NH4+ and NH3A titration is carried out for 25.00 mL of 0.100 M HCl (strong acid) with 0.100 M of a strong base NaOH the titration curve is as shown. Calculate the pH at these volumes of added base solution:(a) 0.00 mL(b) 12.50 mL(c) 25.00 mL(d) 37.50 mL
- A buffer is made with sodium acetate (CH3COONa)and acetic acid (CH3COOH); the Ka for acetic acid is 1.80 * 10-5. The pH of the buffer is 3.98. What is the ratio of the equilibrium concentration of sodium acetate to that of acetic acid?(a) -0.760 (b) 0.174 (c) 0.840 (d) 5.75 (e) Not enough informa-tion is given to answer this question.Calculate the number of grams of ammonium chloride that must be added to 2.00 L of a 0.500 M ammonia solution to obtain a buffer of pH = 9.20. Assume the volume of the solution does not change as the solid is added. Kb for ammonia is 1.80 * 10-5. (a) 60.7 g (b) 30.4 g (c) 1.52 g (d) 0.568 g (e) 1.59 * 10-55. A buffer solution contains 10.0 mmol of formic acid (HCOOH) and 15.0 mmol of formate (HCO0). If the solution pH is 3.95, then what is the Ka of formic acid? (а) 7.5 х 10-5 (b) 1.1 х 104 (c) 4.1 x 102 (d) 1.7 x 10-4