Concept explainers
(a)
Interpretation:
The equilibrium constant of various acid-base reactions has to be calculated.
Concept introduction:
An integer that shows the correlation between quantity of starting material and product of a reversible reaction present at equilibrium is called equilibrium constant.
To give: Equilibrium constant of strong acid reacts with strong base.
(b)
Interpretation:
The equilibrium constant of various acid-base reactions has to be calculated.
Concept introduction:
An integer that shows the correlation between quantity of starting material and product of a reversible reaction present at equilibrium is called equilibrium constant.
To give: equilibrium constant of strong acid reacts with weak base(
(c)
Interpretation:
The equilibrium constant of various acid-base reactions has to be calculated.
Concept introduction:
An integer that shows the correlation between quantity of starting material and product of a reversible reaction present at equilibrium is called equilibrium constant.
To give: equilibrium constant of weak acid (acetic acid) reacts with strong base.
(d)
Interpretation:
The equilibrium constant of various acid-base reactions has to be calculated.
Concept introduction:
An integer that shows the correlation between quantity of starting material and product of a reversible reaction present at equilibrium is called equilibrium constant.
To give: Equilibrium constant of weak acid (acetic acid) reacts with weak base (
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Chemistry: Atoms First
- Weak base B has a pKb of 6.78 and weak acid HA has a pKa of 5.12. a Which is the stronger base, B or A? b Which is the stronger acid, HA or BH+? c Consider the following reaction: B(aq)+HA(aq)BH+(aq)+A(aq) Based on the information about the acid/base strengths for the species in this reaction, is this reaction favored to proceed more to the right or more to the left? Why? d An aqueous solution is made in which the concentration of weak base B is one half the concentration of its acidic salt, BHCl, where BH+ is the conjugate weak add of B. Calculate the pH of the solution. e An aqueous solution is made in which the concentration of weak acid HA twice the concentration of the sodium salt of the weak acid, NaA. Calculate the pH of the solution. f Assume the conjugate pairs B/BH+ and HA/A are capable of being used as color-based end point indicators in acidbase titrations, where B is the base form indicator and BH is the acid form indicator, and HA is the acid form indicator and A is the base form indicator. Select the indicator pair that would be best to use in each of the following titrations: (1) Titration of a strong acid with a strong base. (i) B/BH+ (ii) HA/A (2) Titration of a weak base with a strong acid. (i) B/BH+ (ii) HA/Aarrow_forward7 (a) Describe what happens when each of the following molecules is separately dissolved in water and illustrate with an equation in each case: (i) ethanoic acid (CH₂COOH) (ii) ammonia (NH3) (b) Identify the conjugate acids and bases in the substances mentioned in question 7(a) above. (c) Explain the difference between: (i) a strong acid and weak acid and (ii) a strong base and a weak basearrow_forwardIn the following reactions, identify the Lewis acid and the Lewis base. (a) AlCl3 + Cl¯ → AICI, (b) CH;COOH(aq) + NH3(aq) → CH;COO (aq) + NH (aq) (c) Co³* (aq) + 6F (aq) → [CoF, j*¯ (aq)arrow_forward
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- Methanoic acid is also called formic acid. It has the chemical formula HCOOH(l). It is a colourless fuming liquid that is mainly used as a preservative. It exhibits the following equilibrium in water:HCOOH(aq) + H2O(l) → HCOO–(aq) + H3O+(aq) 3) A 35.0 mL sample of (monoprotic) lactic acid, C3H6O3, is titrated with 20.0 mL of a 4.0 x 10-4 mol/L sodium hydroxide solution. What is the pH of the resulting solution at the equivalence point, if Ka for lactic acid is 1.4 x 10-4? PLEASE HELP THIS IS VERY URGENTarrow_forwardAcetic acid is a weak acid, meaning it does not fully dissociate in water. Instead, there is an equilibrium between the dissolved but undissociated molecule and the component ions: HOAc (aq) + H2O (l) ⇌ H3O+ (aq) + OAc– (aq)OAc– is an abbreviation for the acetate ion, CH3COO–, and H3O+ is the hydronium ion (lone protons, H+ (aq), do not exist!). (d) When starting with completely un-dissociated acetic acid, is it accurate to assume that [HOAc]0 = [HOAc]eq? Why or why not? (e) A highly concentrated acetic acid solution contains 15.0M acetic acid at equilibrium. What are the equilibrium concentrations of the hydronium and acetate ions in this solution? (f) Creating the concentrated acetic acid solution by dissolving liquid HOAc in water raises the temperature of the water by about 5°C from room temperature. At 50°C, do you expect the solution to contain more or less acetate ion OAc– than what you calculated in (c)? Why?arrow_forwardSuppose that, instead of using NaOH, a base such as Ba(OH)2 had been used. What changes in the calculations would then have to be made to determine the molar concentrations of the base?arrow_forward
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