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- (a) Calculate the percent ionization of 0.00800 M butanoic acid (K₂ = 1.5e-05). % ionization = % (b) Calculate the percent ionization of 0.00800 M butanoic acid in a solution containing 0.0610 M sodium butanoate. % ionization = %Why is pH at the equivalence point larger than 7 when youtitrate a weak acid with a strong base? (a) There is excessstrong base at the equivalence point. (b) There is excess weakacid at the equivalence point. (c) The conjugate base that isformed at the equivalence point is a strong base. (d) The conjugate base that is formed at the equivalencepoint reacts with water. (e) This statement is false: the pH isalways 7 at an equivalence point in a pH titration.What is the pH of a solution made by adding 0.65 m of acetic acid (H3CO2H) and 0.30 mol of sodium acetate (H3CO2Na) to enough water to make a 1.0 L solution? (K, = 1.8 x 105) %3D CH3CO2H (aq) + H2O (1) CH3CO2° (aq) + H3O* (aq) 4.74 O 5.08 04.40 8.92
- (a) Calculate the percent ionization of 0.00170 M butanoic acid (K₁ = 1.5e-05). % ionization = 8.96 % (b) Calculate the percent ionization of 0.00170 M butanoic acid in a solution containing 0.0610 M sodium butanoate. X% % ionization -Abuler coAirs the weak acia HA ad is conugate base A. The weak acid has a pK, of 4.36 and the buffler has a pH of 4.92. Part A Which statemeant is true of the relative concentrations of the wweak acid and coniugate base in the bufter? O [HA| = |A"| O [HA| LA | Submit Request Answor Part B Which buffer component wauld you acid to change the pH vi the butfer ta 4.72? O HA(4) Is the salt NaHS acidic, basic, or neutral? Prove your answer.
- The base B has pKb 5.00. (a) What is the value of pKa for the acid BH? (b) At what pH is [BH] [B]? (c) Which is the principal species, B or BH, at pH 7.00? (d) What is the quotient [B]/[BH] at pH 12.00?Which chemical reaction properly demonstrates the protonation of a weak Bronsted-Lowry base in water? H2S (aq) + H20(1) = HS'(aq) + H30*(aq) O C5H5N(aq) + H20(1) = C5H5NH*(aq) + H3O*(aq) C5H5N(aq) + H20(1) = C5H5NH*(aq) + OH (aq) O C5H5N(aq) + H;O*(1) =C5H5NH*(aq) + H2O(1) O H2S(aq) + H20(1) = HS (aq) + OH (aq)3. Buffer solutions are used by the human body to maintain a constant pH for biochemical processes such as enzyme activity. In addition, buffer is used in baby shampoo and soap to maintain the pH, thereby preventing rashes on the baby. Given an ethanoic acid, CH-COОH with Kа %3 1.85 х 105. (а) Calculate the pH of a buffer solution containing 0.150 mol/L ethanoic acid and 0.150 mol/L sodium ethanoate using the Henderson-Hasselbalch equation. Give the proportion (ratio) for [CH;COO-] : [CH;COOH] with the same concentration that we should mix to produce a buffer solution of pH 5.00. (b)
- Ihave some acetic acid that dissociates in water. [CH3COOH] = 0.405 M and [CH3COO]=0.505 M. K3=1.8x10-5. Find the pH=? (3 sig fig)What volume of 2.25-M H2SO4 should be diluted with water to form a 1.25 liters of 1.5 molar of the same acid solution?(14) Which of the following species acts as weak base to neutralize acidity in solution? HCO3 (A) (B) (C) (D) (E) CO2 H2CO3 H20 Na*