A buffer solution was prepared by adding 4.92 g of sodium acetate, NaCH3CO2, to 2.50 x 10^2 mL of 0.170 M acetic acid, CH3CO2H (Ka= 1.8 x 10^-5).
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A buffer solution was prepared by adding 4.92 g of sodium acetate, NaCH3CO2, to 2.50 x 10^2 mL of 0.170 M acetic acid, CH3CO2H (Ka= 1.8 x 10^-5).
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- Does the pH of the solution increase, decrease, or stay the same when you (a) Add solid sodium oxalate, Na2C2O4, to 50.0 mL of 0.015-M oxalic acid? (b) Add solid ammonium chloride to 100. mL of 0.016-M HCl? (c) Add 20.0 g NaCl to 1.0 L of 0.012-M sodium acetate, NaCH3COO?A buffer solution was prepared by adding 4.92 g of sodium acetate, NaCH3CO2, to 2.50 x 10^2 mL of 0.170 M acetic acid, CH3CO2H (Ka= 1.8 x 10^-5). What is the pH of the system if you add 72 mg of NaOH to the 1.00 x 10^2 mL of the prepared buffer solution?The major component of vinegar is acetic acid, CH3COOH. Its Ka is 1.8 × 10-5 . One student used 1.000 M NaOH to titrate 25.00 mL vinegar. At the end point, 21.82 mL NaOH was used. (a) What is the concentration of CH3COOH in vinegar? (b) What is the pH of the solution at the end point? (c) What indicator(s) the student should use in this titration? Explain
- A buffer solution was prepared by adding 4.96 g of sodium acetate,NaCH3CO2, to 2.50x 10^2 mL of 0.170 M acetic acid, CH3CO2H (Ka=1.8 x 10^-5). What is the pH of the system if you add 72 mg of NaOH to the 1.00x 10^2 mL of the prepared buffer solution?Consider the reaction of a 20.0 mL of 0.220 M C;H;NHCI (Ka = 5.9 x 10) with 12.0 mL of 0.239 M CSOH. Write the net ionic equation for the reaction that takes place. What quantity in moles of C;H;NH" would be present at the start of the titration? What quantity in moles of OH" would be present if 12.0 mL of OH were added? -What species would be left in the beaker after the reaction goes to completion? d. What quantity in moles of C,H,NH would be left in the beaker after the reaction goes to completion?You prepared 500 mL buffer solution that contains 0.50 moles monoprotic weak acid (HA) and 0.30 moles conjugate base (NaA). The solution has a pH of 4.20. (a) What is the Kp of the conjugate base, NaA? (b) What is the pH of the buffer solution after adding 400 mL of 0.30 M H,SO4? pH = pKa – log(THA), [A*]
- To simulate the pH of blood, which is 7.4, an undergraduate researcher in a biology lab produced a buffer solution by dissolving sodium dihydrogen phosphate (NaH2PO4, Ka = 6.2 × 10–8) and sodium hydrogen phosphate (Na2HPO4) together in an aqueous solution. What mole ratio of Na2HPO4/NaH2PO4 did she need to use?4. Complete neutralization of 10 mL of hydrochloric acid solution by NaOH 0.1 N in the presence of phenol phthalein until the appearance of purple color (pHf= 9) 15 mL of NaOH is consumed. (a) What is the concentration of hydrochloric acid? (b) Calculate the indicator error.1. If 30.00 ml of a 0.300 mol/L of a weak acid, CH,CO,H (aq), is titrated with a 0.300 mol/L NaOH(aq), a strong base, determine the amount/moles and pH of the remaining acid after K, = 1.8 x 10* (a) 0.00 mL of NaOH is added (b) 10.00 mL of NaOH has been added. O at equivalency point when 30.00ml of NaOH was added. (d) Explain why the pH differs in (b) and (c)
- 1. 30.00 mL of 0.085 M Hydrofluoric acid (HF; Ka = 6.8 x 10-4) is titrated with 0.102 M NaOH. What is the pH of the acid solution before any base is added?You need to show your works.Potassium hydrogen phthalate (KHP) is often used as a primary standard in acid–base titrations. If 19.45 mL NaOH is required to neutralize 0.397 g KHP, what is the concentration of the NaOH?A 25.00 mL sample of 0.1500 M lactic acid was added to a beaker. It was titrated with a 0.1700 M of NaOH in a burette. K₂ =1.4x104 of lactic acid. Calculate the pH when 8.00 mL of NaOH is added in the titration.
