please explain in words and equation.
please explain in words and equation. 5. (10 pts) The pH of a 0.350 M solution...
Calculate the pH in the titration of 45.0 mL of 0.350 M accetic acid by sodium hydroxide after the addition to the acid solution of 10.5 mL of 0.250 M NaOH. The ka of acetic acid is 1.8 x 10^-5
Suppose you titrate 0.310 L of a 0.350 M solution of sodium nicotinate with 6.0 M HCl. Ka for nicotinic acid is 1.5*10-5. What is the pH of the solution before beginning the titration? What is the pH of the solution halfway through the titration? What is the pH at the stoichiometric point? What is a suitable indicator for this titration?
a 1.00 L buffer solution is 0.350 M H2CO3 and 0.500 M KHCO3. Calculate the pH of the buffer solution and the number of moles of base that can be added before the buffer solution is no longer effective. the Ka for H2CO3 is 4.3*10^-7 ( hint : what range of pH is a buffer solution effective?) pka plus or minus?)
Please explain in words and in equations (15 pts) Calculate the pH and the concentration of all the species present at equilibrium for a 1.0E-4 M carbonic acid solution. Ka1: 4.20E-7 Kaz: 4.80E-11 Tulak ach 14.202-7=CACIBOT J A - + H-0)
1. Calculate the pH of a solution prepared by dissolving 0.850 mol of NH3 and 0.350 mol of NH4Cl in water sufficient to yield 1.00 L of solution. The Kb of ammonia is 1.77 × 10-5 (a) 5.137 (b) 4.367 (c) 9.633 (d) 8.781 (e) 8.863 2. A 0.1 M solution of which of the following willl have the highest pH? (a) KCN, Ka of HCN = 4.0x10-10 (b) NH4NO3, Kb of NH3 = 1.8x10-5 (c) NaOAc, Ka of HOAc...
The Ka of propanoic acid (C2H5COOH) is 1.34 × 10-5. Calculate the pH of the solution AND the concentrations of C2H5COOH AND C2H5COO– in a 0.323 M propanoic acid solution at equilibrium. Please explain each step in detail.
please explain. thanks 5. Find the pH and fraction of dissociation for a 0.0SF solution of the weak monoprotic acid HA whose Ka=1.4 x 106. Find the equilibrium molar concentrations of HA, A', H20 and OH, all species, for the solution. Make simplyfing assumptions to avoid solving a quadratic equation State rational for these assumptions
Calculate the [H3O+] and pH of the following polyprotic acid solution: 0.350 M H2C2O4.
please explain how you got these answers!! and me 17) (5 pts) Calculate the pH of a solution that is 0.15 Min ammonia (NH3) and 0.40 ammonium chloride, given the ionization constant of the base, kb, NH3 = 1.76 X 10 equilibrium reaction: NH3(aq) + H20 (1) 2 NH4(aq) + OH' (aq) A) 5.18 B) 8.82 C) 9.25 D) 9.50 E) 9.63 18) (5 pts) By far the most important buffer for maintaining acid-base balance in the blood is the...
Part A A 0.150 M weak acid solution has a pH of 2.97. Find Ka for the acid. Part B Find the percent ionization of a 0.195 M HC2H3O2 solution. (The value of Ka for HC2H3O2 is 1.8×10−5.) Part C Find the pH of a 0.0191 M solution of hypochlorous acid. (The value of Ka for hypochlorous acid is 2.9×10−8.) Part D Find the pH of a 0.014 M solution of HF. (The value of Ka for HF is 3.5×10−4.) Part...