HCN Is a weak acid that dissociates in water. Which statement is completely true? a) HCN...

HCN Is a weak acid that dissociates in water. Which statement is completely true?

a) HCN is the Bronsted-Lowry base in this problem

b) HCN is a conjugate acid in this problem

c) with a Ka value, HCN is a strong acid

d) CN^-1 ion is its conjugte base

e)HCN solutions have a pH value near 11

Solutions

Expert Solution

HCN gives H+

So, it is a Bronsted-Lowry acid

Its conjugate base is CN-

since it is acid, its solution will have pH of less than 7

Answer: d

queen_honey_blossom answered 2 years ago

Next > < Previous

Related Solutions

Hydrocyanic acid (HCN) is a weak acid that dissociates in water as follows. HCN(aq) + H2O(l)...

Hydrocyanic acid (HCN) is a weak acid that dissociates in water as follows. HCN(aq) + H2O(l) equilibrium reaction arrow H3O+(aq) + CN −(aq) The acid-dissociation constant (Ka) for hydrocyanic acid is 6.2 ✕ 10−10. Calculate the percent ionization (percent dissociation) if the initial concentration of hydrocyanic acid was 0.29 M.

hcn is a weak acid that ionizes in water to a small extent. Addition of NaCl...

hcn is a weak acid that ionizes in water to a small extent. Addition of NaCl to an aqueous solution of hcn will cause the equilibrium of the reaction to shift towards the ______due to the presence of a ________. common ion reactant product spectator ion

Hydrocyanic acid, HCN, is a weak acid. Write a net ionic equation for the reaction of...

Hydrocyanic acid, HCN, is a weak acid. Write a net ionic equation for the reaction of aqueous hydrocyanic acid and aqueous sodium hydroxide.

Cyanic acid (HCN) is a weak acid with a Ka value of 6.2 ✕ 10-10. Calculate...

Cyanic acid (HCN) is a weak acid with a Ka value of 6.2 ✕ 10-10. Calculate the pH of a 1.26 M solution of sodium cyanide - NaCN(aq).

Consider the following dissociation of the weak acid, HCN: HCN(aq) ⇌ CN−(aq) + H+(aq) K =...

Consider the following dissociation of the weak acid, HCN: HCN(aq) ⇌ CN−(aq) + H+(aq) K = 6.2×10-10 A solution is made with an initial concentration of 2.60 M HCN. At equilibrium, what is the concentration of H+ ions in solution? (Hint: You may use the 5% approximation.) ?M

Trichloroacetic acid dissociates partially in water according to the equilibrium below. What is the percentage of...

Trichloroacetic acid dissociates partially in water according to the equilibrium below. What is the percentage of molecules dissociated in a 1.00 molal solution of trichloroacetic acid in water if the measured freezing point is -2.53C? The freezing point and Kf for water are 0.00C and 1.86 C-kg/mol, respectively. CCl3CO2H(aq) -> <- (Equalibrium arrows) CCl3CO2 1- (aq) + H+ (aq) How do I set up and Solve

1. The degree to which a weak base dissociates is given by the base-ionization constant, Kb....

1. The degree to which a weak base dissociates is given by the base-ionization constant, Kb. For the generic weak base, B B(aq)+H2O(l)⇌BH+(aq)+OH−(aq) this constant is given by Kb=[BH+][OH−][B] Strong bases will have a higher Kb value. Similarly, strong bases will have a higher percent ionization value. Percent ionization=[OH−] equilibrium[B] initial×100% Strong bases, for which Kb is very large, ionize completely (100%). For weak bases, the percent ionization changes with concentration. The more dilute the solution, the greater the percent...

HCN gas, a powerful respiratory inhibitor, is highly toxic. It is a very weak acid (Ka...

HCN gas, a powerful respiratory inhibitor, is highly toxic. It is a very weak acid (Ka = 6.2 x 10-10) when dissolved in water. If a 50.00-mL sample of 0.100 M HCN is titrated with 0.100 M NaOH, calculate the pH of the solution: a. before the titration starts. b. after 8.00 mL of 0.100 M NaOH has been added. c. at the half-way point of the titration. d. at the equivalence point of the titration. e. after 52.00 mL...

The reaction of the weak acid HCN with the strong base KOH is: HCN(aq)+KOH(aq)-->HOH(l)+KCN(aq) To compute...

The reaction of the weak acid HCN with the strong base KOH is: HCN(aq)+KOH(aq)-->HOH(l)+KCN(aq) To compute the pH of the resulting solution if 54mL of 0.79M HCN is mixed with 2.0 × 10^1 mL of 0.32 KOH we need to start with the stoichiometry. Let\'s do just the stoich in steps:. a)How many moles of acid? b)How many moles of base? c)What is the limiting reactant? d)How many moles of the excess reagent after reaction? e)What is the concentration of...

c. What is the most important weak acid in water?

Subjects