Calculate the pH of a buffer solution made by mixing 300 mL of 0.3M acetic acid, CH;COOH, and 200-mL of 0.2 M of its salt sodium acetate, CH3COONA, to make 500 mL of solution. Ka for CH3COOH = 1.76x 10-5 O 4.4 O 5.0 6.3 2 3.4

Aspirin (C 9H 8O 4) is a weak monoprotic acid (K a = 3.3 x 10-4). You are analyzing a samplefor a pharmaceutical company with a quantitative titration and dissolve 10 tablets, eachcontaining 200 mg of aspirin, in 150 mL of water.a) Determine the pH of this solution.b) Determine the pH of the solution after you have added 20.0 mL of 0.500 M NaOH.

A solution is prepared that is initially 0.13M in acetic acid (HCH3CO₂) and 0.24M in potassium acetate (KCH3CO₂). Complete the reaction table below, so that you could use it to calculate the pH of this solution. Use x to stand for the unknown change in initial change final [HCH,CO₂] 0 [H₂0]. You can leave out the M symbol for molarity. [cH,co,] 0 L [H₂O] 0 0 0 plo X G

A buffer is made by adding 0.18 mol/L of sodium propanoate (NaPr) to 0.12 mol/L solution of propanoic acid (HPr, K«= 1.3 x 105). Assume the volume of the solution to be 1.0 L. a) Write the chemical equation for the acid hydrolysis reaction. | b) What is the acid-base conjugate pair that governs the pH of the buffer? c) Calculate the pH of the buffer. Be sure to justify and validate any approximations used.

If the buffer prepared by mixing 0.30 M C,H;NH;HCI(aq) with 0.50 M CH;NH, in the previous question was attacked with the addition of 0.20 M NaOH(aq) determine the pH after the attack. C, H NH2 + H,O = C,H, NH, H + OH K, = 6.4 x 10-4 O 10.81 D 13.00 O 8.88 O None of these 0 11.66

An analytical chemist is titrating 111.3 mL of a 0.2800 M solution of ammonia (NH, with a 0.3500 M solution of HIO,. The p K, of ammonia is 4.74. Calculate 3' the pH of the base solution after the chemist has added 99.0 mL of the HIO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HIO, solution added. Round your answer to 2 decimal places.

A solution prepared by mixing 1.73 of propionic acid (HC3H5O2) and 0.53 g of NaOH in water (Ka propionic acid = 1.4 x 10^-5 ). a) calculate the moles of the reactants. Which is the limiting reactant? b) What will be the moles of the products? What are the moles of the excess reactant? c) calculate the pH of the acid buffer

A buffer solution is made such that the initial concentrations of lactic acid (HC3H5O3) and the lactate ion (C3H­O­-) are 0.600 M and 0.620 M, respectively. What is the resulting pH if 300.0 mL of 0.100 M potassium hydroxide is added to 0.600 L of the buffer solution? (The Ka of HC3H5O3 is 1.4 x 10-4.) Answer not in scientific notation

A solution is prepared by mixing 500 mL of 0.10 M NaOCI and 500 mL of 0.20 M HOCI. What is the pH of this solution? [Ka(HOCI) = 3.2 × 10-8] 4.10 O 7.00 7.19 O 7.49

propionic acid, ?a=1.34×10−5,Ka=1.34×10−5, 3.00 M sodium propionate, CH3CH2COONa   1. The final volume of buffer solution must be 100.00 mL and the final concentration of the weak acid must be 0.100 M. Based on this information, what mass of solid conjugate base should the student weigh out to make the buffer solution with a pH of 5.00? ( in g) 2. Based on this information, what volume of acid should the student measure to make the buffer solution? (in ml)