Calculate the change in pH when 69.0 mL of a 0.660 M solution of NaOH is added to 1.00 L of a solution that is 1.00 M in sodium acetate and 1.00 M in acetic acid.
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- l See Periodic Table O See Hint Calculate the change in pH when 41.0 mL of a 0.500 M solution of NaOH is added to 1.00 L of a solution that is 1.00 M in sodium acetate and 1.00 M in acetic acid. 4.798Calculate the pH change that results when 15 mL of 2.0 M HCI is added to 580. mL of each of the following solutions (a) pure water 4.0-5.70 (b) 0.10 M CH3COO 4.04.28 (c) 0.10 M CH3COOH 4.0 (d) a solution that is 0.10 M in each CH3COO and CH3COOH. 4.0A buffer solution contains 0.433 M NaHSO3 and 0.291 M K2SO3. If 0.0340 moles of sodium hydroxide are added to 225 mL of this buffer, what is the pH of the resulting solution ? (Assume that the volume does not change upon adding sodium hydroxide) ( Please type answer note write by hend )
- 2. (a) Calculate the pH after 0.10 mol NaOH is added to 1.00 L of a solution that is 0.6 M HF and 1.00 M KF.A buffer solution contains 0.248 M KH2PO4 and 0.482 M Na2HPO4.If 0.0383 moles of hydrobromic acid are added to 225 mL of this buffer, what is the pH of the resulting solution ? Please type answer not write by hendCalculate the pH change that results when 11 mL of 5.1 M NaOH is added to 790. mL of each the following solutions. Use the Acid-Base Table. (a) pure water 4.0 5.84 (b) 0.10 M NH4CI 4.0 5.43 (c) 0.10 M NH3 4.0✔ X (d) a solution that is 0.10 M in each NH4+ and NH3 4.0✔
- A buffer solution could be made by mixing equal amounts of citric acid and a solution containing. would resist When a small amount of strong acid or base is added, this buffer The statements above are completed by ཤ (-) (-C,H,O(C00), tay ila pH change (aq) i-C,H,O(COO), (aq) О -C,H,O(COOH),COO) О i-C,H,O(COOH),C00(a) it an equilibrium shift -a pH change -an equilibrium shiftA 93.0 mL sample of 0.0100 M HIO4 is titrated with 0.0200 M LIOH solution. Calculate the pH after the following volumes of base have been added. (a) 14.4 mL pH = 2.57 (d) 47.4 mL pH = X X (b) 44.2 mL pH = (e) 78.1 mL pH = X X (c) 46.5 mL pH = XCalculate the pH of the solution that results when 20.0 mL of 0.1750 M formic acid is: [Ka = 1.8 x 10-4] (a) diluted to 45.0 mL with distilled water. (b) mixed with 25.0 mL of 0.140 M NaOH solution. (c) mixed with 25.0 mL of 0.200 M NaOH solution. (d) mixed with 25.0 mL of 0.200 sodium formate solution
- CuFrent Attempt in PPogress A buffer is prepared by mixing 48.9 g of NH3 and 48.9 g of NH,Cl in 0.683 L of solution. What is the pH of this buffer, and what will the pH change to if 7.68 g of HCI is then added to the mixture? Your answer is correct. pH of this buffer= 9.62 Hint Your answer is incorrect. The pH change = i (in case of decreasing pH the answer should be negative). Hint MacBook AirCalculate the pH change that results when 15 mL of 2.7 M HCI is added to 600. mL of each of the following solutions. Use the Acid-Base Table. (a) pure water 4.0 -5.82 (b) 0.10 M CH3COO- 4.0 4.43 (c) 0.10 M CH3COOH 4.0 X (d) a solution that is 0.10 M in each CH3COO and CH3COOH. 4.0When 14.08 mL of 0.1594 M NaOH is added to 25.00 mL of 0.1235 M HX (an unknown weak acid), the resulting pH is 4.7. What is the Ka of the unknown acid?