What is the pH when 3.7 g of sodium acetate, NaC2H3O2, is dissolved in 150.0 mL of water? (The Ka of acetic acid, HC2H3O2, is 1.8×10^−5).
What is the pH when 3.7 g of sodium acetate, NaC2H3O2, is dissolved in 150.0 mL...
Part A What is the pH when 5.3 g of sodium acetate, NaC2H3 O2, is dissolved in 500.0 mL of water? (The Ka of acetic acid, HCa H3 O2, is 1.8 x 10-5) Express your answer to two decimal places. να ΑΣφ ? pH= Submit Request Answer
500 mg of sodium acetate is dissolved in 500.0 mL of de-ionized water. Calculate the pH of this solution. MM(sodium acetate) = 82.0324 g/mol, Ka(acetic acid) = 1.75 x 10-5
Calculate the mass of solid sodium acetate trihydrate, NaC2H3O2. ⋅ 3H2O, required to mix with 100.0 mL of 1.0 M acetic acid to prepare a pH 4 buffer. The Ka of acetic acid is 1.8 × 10–5
2. What is the pH when 5.3 g of sodium acetate, NaC H302, is dissolved in 100.0 mL of water? (The K, of acetic acid, HC H302, is 1.8x10-))
During this part #3 of the lab, you will make 2 acetic acid buffer solutions (HC2H3O2/NaC2H3O2) of the same pH (pH = 4.0), but with different concentration of the components. Use the Henderson -Hasselbalch equation to perform the following calculations. The Ka of acetic acid is 1.8 x 10-5 M. a. Buffer A: Calculate the mass of the solid sodium acetate (NaC2H3O2) required to mix with 100 ml of 0.1 M acetic acid (HC2H3O2), to prepare a pH 4 buffer....
6. What mass of sodium acetate (NaCH3COO) should be dissolved in 250.0 mL of 0.30 M acetic acid (CH3COOH) to form a buffer of pH 5.0? [Ka for acetic acid is 1.8 × 10−5 ] (a) 11 g (b) 8.0 g (c) 7.5 g (d) 5.0 g (e) 1.4 g
Calculate the pH of a solution made by adding 42 g of sodium acetate, NaCH3COO, to 22 g of acetic acid, CH3COOH, and dissolving in water to make 300. mL of solution. Hint given in feedback. The K, for CH3COOH is 1.8 x 10-5 M. As usual, report pH to 2 decimal places. Answer: Calculate the pH of a solution made by adding 59 g of sodium acetate, NaCH3COO, to 22 g of acetic acid, CH3COOH, and dissolving in water...
A buffer solution is prepared by dissolving 1.000 g of sodium acetate (CH3COONa) into 100.00 mL of a 0.100 M solution of acetic acid. Then 2.00 mL of a 1.00 M solution of hydrochloric acid is added to the acetic acid/sodium acetate buffer solution. The Ka of acetic acid is 1.8 × 10−5. What is the pH of HCl?
A solution is prepared by dissolving 1.100 g of sodium acetate (CH3COONa) into 100.00 mL of a 0.110 M solution of acetic acid. The Ka of acetic acid is 1.8 × 10−5. What is the pH of the solution?
" Determine the amount of sodium acetate needed to prepare 50.0 mL of acetic acid/sodium acetate buffer having a H of 5.0 using approximately 0.100 M acetic acid. Check the concentration of the acetic acid in the laboratory and use this exact concentration for your calculation. For acetic acid Ka= 1.8 x 105." The answer is 0.75g NaC2H3O2. But I need to show the equation steps. Any help?