What is the pH of a 1.2 M pyridine solution that has Kp = 1.9 x 10 9? The equation for the dissociation of pyridine is C5H5N(aq) + H2O(1)= C5H5NH*(aq) + OH"(aq). 10.68 9.68 8.72 4.32
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- The pH of an aqueous solution of 0.400 M hydrocyanic acid, (Ka (HCN) = 4.00 × 10-10) isThe base protonation constant K, of lidocaine (C14H2]NONH) is 1.15 × 10 Calculate the pH of a 0.73 M solution of lidocaine at 25 °C. Round your answer to 1 decimal place. pH = ]CH3CH2CO2H , Ką = 1.3 x 105 CH3CH2CO2 , Kp = 7.7 x 10-10 F, Kp = 1.4 x 10-11 HF , Ką = 7.2 x 10-4 For the reaction between propanoic acid (CH3CH2CO2H) and a solution containing fluoride ions (F"): (a) The name of the conjugate base produced is (b) The name of the conjugate acid produced is (c) The reaction is favoured (write 'reactant' or 'product'), because the reactants are the (write 'weaker' or 'stronger') set of acid and base.
- Write the expression for K, and K, for the reaction PH;BCl,(s) = PH;(e) + BCl(g) 1.نقطتان )2( The pH of a 1.00 M Solution -1 of Nitrous acid HNO2 (pKb =10.6) is25. (a) What is a Brønsted-Lowry acid? (b) What is a Brønsted-Lowry base? (c) Use the following chemical equation to explain these concepts and (d) to identify the conjugate acid-base pairs. Point form is both accepted and expected for this question. ( + CO3 (aq) (aq) 2- HCO3 (ag) + S² = HS, (aq)
- The base protonation constant K, of allantoin (C4H,N,O,NH,) is 9.12 x 10 °. 9. 3 Calculate the pH of a 0.47 M solution of allantoin at 25 °C. Round your answer to 1 decimal place. pH = | ?When NaCLO(s) dissolves in water it dissociates as follows NaCLO(s) + H2O(l) →Na+(aq) + CLO-(aq) is the conjugate base of the weak acid, hypochlorous acid, as follows: CLO- (aq) + H2O(l) ⇌HCLO(aq) + OH- (aq) How many grams of NaCLO must be added to 2.00 L of water to make a solution with a pH of 10.50? Kb = [HCLO-][OH-]/[CLO-] = 3.3x10−7 a) 0.46 grams b) 23 grams c) 0.31 grams d) 46 gramsis a weak base with a p K, of 7.94. Calculate the pH at 25 °C of a 0.33 M solution of lidocaine HCl (C4H NONH,CI). Note that lidocaine (C14H21NONH) Round your answer to 1 decimal place. pH =
- Phosphoric acid, H3PO4, is a triprotic acid, for which Ka1 =7.2 x 103, Ka2 = 6.3 × 10-8 and Ka3 = 4.2 x 1013. What is the value of K for the following equation. HPO42 (aq) + H20(1) Z H,PO4 (aq) + OH"(aq) Express your answer in scientific notation rounded to three significant figures.Identify the acid, base, conjugate acid and conjugate base in the following reactions: HF (aq) + H,O (1) H;O* (aq) + F ¯(aq) CH;CH,NH, (aq) + H,O (1) CH;CH,NH;" (aq)+OH (aq)Consider the dissociation of hydrocyanic acid in aqueous solution HCN - CN + H* for which K, is 4.9 x 101°. (i) Find the pH of a solution initially 102 M in HCN, and the degree of dissociation of the HCN, a. (ii) To this solution is added more CN' until [CN'] = (0.1 M. What is the new pH of the solution? (ii) Without making a new numerical cakculation, explain qualitatively how the degree of dissociation would change if the solution is diluted.