Concept explainers
If you mix equal concentrations of reactants and products, which of the following reactions proceed to the right and which proceed to the left?
(a)
(b)
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Chapter 14 Solutions
General Chemistry: Atoms First
- A chemist wanted to determine the concentration of a solution of lactic acid, HC3H5O3. She found that the pH of the solution was 2.60. What was the concentration of the solution? The Kd of lactic acid is 1.4 104.arrow_forwardIonization of the first proton from H2SO4 is complete (H2SO4 is a strong acid); the acid-ionization constant for the second proton is 1.1 102. a What would be the approximate hydronium-ion concentration in 0.100 M H2SO4 if ionization of the second proton were ignored? b The ionization of the second proton must be considered for a more exact answer, however. Calculate the hydronium-ion concentration in 0.100 M H2SO4, accounting for the ionization of both protons.arrow_forwardWrite the chemical equation and the expression for the equilibrium constant, and calculate Kb for the reaction of each of the following ions as a base. (a) sulfate ion (b) citrate ionarrow_forward
- For each of the following reactions, predict whether the equilibrium lies predominantly to the left or to the right. Explain your predictions briefly. (a) NH4+(aq) + Br(aq) NH3(aq) + HBr(aq) (b) HPO42(aq) + CH3CO2(aq) PO43(aq) + CH3CO2H(aq) (c)[Fe(H2O)6]3+(aq) + HCO3(aq) [Fe(H2O)5(OH)]2+(aq) + H2CO3(aq)arrow_forwardFor each of the following salts in water, predict whether the pH will be greater than, less than, or equal to 7. (a) KBr (b) NH3NO3 (c) AlCl3 (d) Na2HPO4arrow_forwardIdentify and justify the Bronsted-Lowry acid in the reaction: NH3 + HBr à NH4Br(a) NH3 because it is a proton donor (b) HBr because it is a proton donor(c) NH3 because it is a proton acceptor (d) HBr because it is a proton acceptorarrow_forward
- - pH of Saliva The pH of saliva is normally in the range of 6.4 to 7.0. However, when a person is ill, the person's saliva becomes more acidic. (a) When Marco is sick, he tests the pH of his saliva and finds that it is 5.5. What is the hydrogen ion concentra- tion of his saliva? (b) Will the hydrogen ion concentration in Marco's saliva increase or decrease as he gets better? (c) After Marco recovers, he tests the pH of his saliva, and it is 6.5. Was the saliva more acidic or less acidic when he was sick?arrow_forwardThe odor of spoiled butter is due in part to butanoic acid (HC4H7O2) which results from the breakdown of the fat in butter. A 0.100M solution of butanoic acid is 1.23% ionized. a) Write the chemical equation for the ionization of this acid in water. b) Write the Ka expression for this acid. c) What is the equilibrium concentration of each product and the reactant? d) What is the value of Ka? e) What is the pH of the solution?arrow_forwardWhat is the effect on the concentration of hydrofluoric acid, hydronium ion, and fluoride ion when the following are added to separate solutions of hydrofluoric acid? The equation for the equilibrium is: HF(aq) + H2O(l) ⇌ H3O+(aq) + F−(aq) HCl KF NaCl KOH HFarrow_forward
- Calculate the pH and the pOH of each of the following solutions at 25°C for which the substances ionize completely. (Assume K 1.01x 10-14.) (a) 0.215 M HCI pH 4.0 pOH 4.0 (b) 0.0126M NAOH pH 4.0 РОН 4.0 (c) 2.9 M HNO3 pH 4.0 РОН 4.0 (d) 0.0038 M Ca(OH)2 pH 4.0 РОН 4.0 Supporting Materials Periodic Table Constants and I Supplemental Data Factors Additional Materials Section 14.2 80 000 000 DII DD esc F10 F5 F6 F7 F8 F9 F1 F2 F3 F4arrow_forwardThe values of K a for hydrozoic acid ( HN 3) and hypobromous acid (HB1O) are given below. HN3 Ką = 1.9 x 10-5 HBrO Ka = 2.0 x 10-9 If we mix 0.50 mol HN 3 and 0.50 mol NaBrO into a 1-L aqueous solution, which of the following statements is correct concerning the final solution at cquilibrium after mixing? O a. The pH of the final solution is greater than 7 because Ką (HN3) K½(BrO"). O . The pH of the final solution is equal to 7 because the neutralization reaction between HN3 and NaBro. d. The pH of the final solution is less than 7 because Ką (HN3) > Kh( BrO" ). O e. The pH of the final solution is less than 7 because Ką (HN3) < K,( BrO" ).arrow_forwardFor each chemical reaction in the table below, decide whether highlighted reactant reaction Bronsted-Lowry Bronsted-Lowry neither acid base NH,(aq) + H,O() → NH, (aq) + OH (aq) NH3(aq) + H,O() - NH (aa) + OH (a) NH, (aq) + ОН (ад) NH,(aq) - H,O() NH (aq) + – H,|() + OH (aq) NH, (aq) Explanation Check 2022 M 80 Farrow_forward
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