a) HCl(aq) + H2O(l) -------------> H3O+(aq) + Cl-(aq) HCl is strong acid so dissociates completely
b) H2SO3(aq) + H2O(l) <-----------> HSO3-(aq) + H3O+(aq) H2SO3 is weak acid so dissociates partialy
for weak acids
Ka = [H3O+][HSO3-]/[H2SO3]
c) HNO3(aq) + H2O(l) ------------> H3O+(aq) + NO3-(aq) HNO3 is strong acid so dissociates completely.
d) HCN(aq) + H2O(l) <--------------> CN-(aq) + H3O+(aq) HCN is weak acid so dissociates partially
Ka = [H3O+][CN-] / [HCN]
8. Please write out the reaction for each of the following acids when dissolved in water....
1. Write the equilibrium expression for the autoionization of water. Using this expression define the terms acid and base and pH. 2. Calculate the pH, pOH, Ka, Kb, pKa, and pKb for a 0.082M solution of triethylamine. 3. Calculate the pH, pOH, Ka, Kb, pKa, and pKb for a 1.570 M solution of hydrogen cyanide. 4. The acid-dissociation constant for hypochlorus acid is 3.0 X 10-8. Calculate the concentrations of H3O+, CIO-, and HCIO at equilibrium if the initial concentration...
Write the Ka or Kb expression for each of the following compounds upon reaction with water. a. HCl b. NH3 c. HNO3 d. KOH
Rank the following acids in order of increasing acid strength when dissolved in water. EXPLAIN your ranking using both inductive effect (think about the O atoms) and the stability of the product (draw all the resonances of the product, think about the number of resonances) HMnO4, H3AsO4, H2SO3, H2SO4
Write the balanced chemical equation for the reaction of the weak acid HCN with water. Include the phase of each species. chemical equation: HCNaq +H,9, H,09 + CNaq Complete the K, expression for this reaction. Answer Bank Ka= [ H0] (CN) [,0] HCN] [OH) [H]
please help with #3 a and b 3. Write the dissociation reaction for the following acids in water. Use appropriate arrow symbols. Label the Bronsted-Lowry acid, base, conjugate acid, and conjugate base for each, then draw lines to connect the appropriate conjugate pairs: (4 pts) a. C.H.COOH (benzoic acid) + H20 b. HCI (hydrochloric acid) + H20
For each of the following metals, write their balanced reaction for when they react with HNO3 a) Al(s) b) k(s) c) Na(s) d) Mg(s)?
4. Equal moles of the indicated acids are dissolved in the ammon of he acid be beakers below. In which solution will the percent ionization of water shown in the of the acid be the lowest? Op -HC a. All have equal percent ionization of acid. c.Ⅳ e. 5. For a 0.05 M H2SOs solution, which of the following relationships is true? b. [SO327 키HS037 C [HSOs 1> [H2SO3] dHSH) 6. Which of the following reactions is associated with the...
1. Write the equations for the reaction of the following Bronsted acids with water: (a) H2S (b) HC2O4- (c) HSO3- 2. Write equations for the reactions of the following Bronsted bases with water: (a) PO4 3- (b) N2H4 (c) H2C6H5O7- 3. In each of the following questions, assume that there is no volume change when HCl is added to water in part (a) or the phosphate buffer in part (c). (a) Calculate the pH when 0.129 moles of HCl are added...
3. Identify the metal or nonmetal oxides that react with water to make the following acids. Write the balanced equation in each case. (a) K(OH) (b) Al(OH)3 (c) HNO3 (d) H2CO3 (e) Ba(OH)2
1. Write the dissociation reaction and the corresponding K, equilibrium expression for each of the following )HCN bHOC.H 2. You may need Table 14.2 to answer the following questions a) Which is the stronger base, CT or HO b) Which is the stronger base, HiO or NO? c) which is the stronger base, Cr or OCH,7 3. Calculate the [H"1 of each of the following solutions at 25 C. Identity each solution as neutral, acidic, or basic. a) [OH] ....