(a)
Interpretation:
The amphiprotic character of
Concept Introduction:
A species that can acts as both proton donor or and also as a proton acceptor is known as amphiprotic. This reacts with both acid and base. Important character of the amphiprotic species is that it has hydrogen atoms which can be donated.
Proton donor is referred as Bronsted acid while proton acceptor is referred as Bronsted base. In a reaction, where a proton is alone transferred from one species to another species is known as Proton-transfer reaction.
Generally acid donates proton to form conjugate base. As donation of proton takes place, the conjugate base will have fewer hydrogen ions than that is present in acid. Base accepts protons to form conjugate acid. As proton is accepted, the conjugate acid will have more hydrogen ions than that of the base from which it is formed.
(b)
Interpretation:
The amphiprotic character of
Concept Introduction:
Refer part (a).
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Chapter 6 Solutions
ACHIEVE/CHEMICAL PRINCIPLES ACCESS 1TERM
- For the following acid-base reaction, (1) predict the products, showing both reactants and products complete Lewis structures and arrows showing electron flow; (2) label each structure with the lowing: Bronsted acid, Bronsted base, conjugate acid, conjugate base; (3) give a brief definition of a ronsted acid and Bronsted base; (4) predict the direction of the equilibrium and justify your answer. HC0OH + CH3 Nta PRん106Y pkb = 3.36arrow_forwardCalculate the pH (aq., 25 oC) of a 0.100 M triethylamine ((C2H5)3N) solution whose Kb = 1.02 x 10–3.arrow_forwardWrite the chemical reaction for the conversion of CO2 to HCO3-, including the enzyme that catalyzes the reaction.arrow_forward
- Determine the pH of each of the following solutions (Ka and Kb values can be found in the appendices of your textbook or online): (a) 0.045 M hypochlorous acid; (b) 0.0068 M phenol; (c) 0.080 M hydroxylamine.arrow_forwardConsider the titration of a 50.00 mL sample of 0.500 M hydrazoic acid, HN3, with 0.500 M NaOH (aq., 25 oC). The Ka HN3 = 4.50 x 10–4. What is the pH of the solution after 15.00 mL of NaOH has been added?arrow_forwardThe active ingredient of bleach such as Clorox is sodium hypochlorite (NaClO). Its conjugate acid, hypochlorous acid (HClO), has a Ka of 3.0 × 10–8. (a)The undiluted bleach contains roughly 1 M NaClO. Calculate the pH of 1 M NaClO solution. (b)Some applications require extremely diluted bleach solution, such as swimming pools. Suppose the solution in (a) is diluted by 10,000 -fold. Calculate the pH of the diluted solution, and demonstrate that you can still neglect the autoionization of water in your calculation. (c)Suppose the solution in (a) is diluted by 1million-fold, briefly explain how your approach will be different. Write the equation with [H3O+] as the unknown, but you do not need to solve it.arrow_forward
- Ethylammonium chloride, CH;CH;NH3CI, is an acidic salt. (i) Write equations to show the dissolving of CH;CH2NH;CI in water and the further reaction of the ethylammonium ion. (ii) Calculate the pH of a 0.218 mol L1 solution of ethylammonium chloridearrow_forwardThere are many organic acids and bases in our cells, and their presence modifies the pH of the fluids inside them. It is useful to be able to assess the pH of solutions of acids and bases and to make inferences from measured values of the pH. A solution of equal concentrations of lactic acid and sodium lactate was found to have pH= 3.08. (a) What are the values of pKa and Ka of lactic acid? (b) What would the pH be if the acid had twice the concentration of the salt?arrow_forwardThe active ingredient of bleach such as Clorox is sodium hypochlorite (NaClO). Its conjugate acid, hypochlorous acid (HClO), has a Ka of 3.0 × 10–8. (a) The undiluted bleach contains roughly 1 M NaClO.Calculate the pH of 1 M NaClO solution. (b) Some applications require extremely diluted bleach solution, such as swimming pools. Suppose the solution in (a) is diluted by 10,000-fold. Calculate the pH of the diluted solution, and demonstrate that you can still neglect the autoionization of water in your calculation. (c) Suppose the solution in (a) is diluted by 1 million-fold, briefly explain how your approach willbe different. Write the equation with [H3O+] as the unknown, but you do not need to solve it.arrow_forward
- Calculate the pH of 0.225 M RbOH(aq).arrow_forwardCalculate the pH of a solution prepared by dissolving 1.15g of sodium acetate, CH3COONa, in 95.5 mL of 0.10 M acetic acid, CH3 COOH(aq). Assume the volume change upon dissolving the sodium is negligible. Ka of CH3COOH is 1.75 x 10-5.arrow_forwardWhat is the conjugate acid of potassium hydrogen phosphate, K2HPO4?arrow_forward
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