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.

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queen_honey_blossom answered 2 years ago

Hydrocyanic acid will set up the following equilibrium when dissolved in water: HCN(aq) + H2O(l) <-->...

Hydrocyanic acid will set up the following equilibrium when dissolved in water: HCN(aq) + H2O(l) <--> CN-(aq) +H3O+(aq) a) calculate the pH of a .123 M solution of hydrocyanic acid ANSWER: pH = 5.01 b) To 500mL of the solution in part (a) is added 5.00g of solid NaCN. Calculate the pH of new solution. Assume no volume change has occured. c) If one were to add 10.00mL of a .100M NaOH solution to the solution prepared in part (b),...

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

Dissociation Constant For the dissociation reaction of a weak acid in water, HA(aq)+H2O(l)?H3O+(aq)+A?(aq) the equilibrium constant...

Dissociation Constant For the dissociation reaction of a weak acid in water, HA(aq)+H2O(l)?H3O+(aq)+A?(aq) the equilibrium constant is the acid-dissociation constant, Ka, and takes the form Ka=[H3O+][A?][HA] Weak bases accept a proton from water to give the conjugate acid and OH? ions: B(aq)+H2O(l)?BH+(aq)+OH?(aq) The equilibrium constant Kb is called the base-dissociation constant and can be found by the formula Kb=[BH+][OH?][B] When solving equilibrium-based expression, it is often helpful to keep track of changing concentrations is through what is often called an...

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...

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.

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

Is hydrocyanic acid (HCN) more soluble in water or in carbon disulfide (CS2)? Why?

Sulfur dioxide is quite soluble in water: SO2(g)+H2O(l)⇌H2SO3(aq)K=1.33 The H2SO3 produced is a weak diprotic acid...

Sulfur dioxide is quite soluble in water: SO2(g)+H2O(l)⇌H2SO3(aq)K=1.33 The H2SO3 produced is a weak diprotic acid (Ka1 = 1.5×10−2, Ka2 = 6.3×10−8) Part A Calculate the pH in a solution prepared by continuously bubbling SO2 at a pressure of 1.00 atm into pure water. Express your answer using two decimal places. Part B Calculate the concentration of H2SO3. Express your answer using three significant figures. Part C Calculate the concentration of HSO3−. Express your answer using two significant figures. Part...

The enthalpy of reaction for HCN(aq) + OH-(aq) -> CN-(aq) + H2O(l) is -12.1 kJ/mol. Assuming...

The enthalpy of reaction for HCN(aq) + OH-(aq) -> CN-(aq) + H2O(l) is -12.1 kJ/mol. Assuming that the correct enthalpy of reaction of the experiment is -54.0 kJ/mol, calculate the enthalpy change for the ionization of HCN: HCN(aq) -> H+(aq) + CN-(aq) Be sure to report your answer to the correct number of significant figures. ΔH = ____ kJ/mol

a) identify the conjugate acid-base pairs for the following reaction: H2O (aq) + CN- (aq)--->HCN (aq)+OH-...

a) identify the conjugate acid-base pairs for the following reaction: H2O (aq) + CN- (aq)--->HCN (aq)+OH- (aq) b) give the conjugate acid of HSO4- and PO4 -2 c) give the conjugate base of HCLO4 and H3O+

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