PLEASE answer 7 and 8 Calculate the pH of a solution prepared by dissolving 0.150 mol...
1. A solution is prepared by dissolving 0.23 mol of butanoic acid and 0.27 mol of sodium butanoate in water sufficient to yield 1.00 L of solution. The addition of 0.0O5 mol of HCI to this buffer solution causes the plH to drop slightly. The pH does not decrease drastically because the HCl reacts with the present in the buffer solution. The Ka of butanoic acid is 1.36x 10-3 A) H20 в) Нзо+ butanoate ion D butanoic acid AlE) This...
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...
Calculate the pH of a solution prepared by dissolving 0.050 mol of benzoic acid (HA) and 0.50 mol of sodium benzoate (A-) in water sufficient to yield 1.00 L of solution. The Ka of benzoic acid is 6.30 x 10-5 A. 5.20 B. 1.30 C. 7.00 D. 3.20 E. 4.20
Calculate the pH of a buffer solution prepared by dissolving 1.79 mol of HF and 2.26 mol of NaF in water to make a total volume of 1.25 L of solution. The Ka of HF is 6.8*10^-4. A) 3.57 B) 3.47 C) 3.27 D) 3.37 E) 3.68 Please let me know what answer is correct and how to work it. Thank You!
Calculate the pH of a solution that is prepared by dissolving 0.470 mol of hydrocyanic acid (HCN, Ka = 6.17×10-10) and 0.180 mol of nitrous acid (HNO2, Ka = 4.60×10-4) in water and diluting to 2.30 L. Also, calculate the equilibrium concentrations of HCN, CN-, HNO2, and NO2-. Do not make an approximation unless the initial acid concentration is greater than 1000 × Ka. (Hint: The pH will be determined by the stronger acid of this pair.) pH = [HCN]...
calculate the pH in a solution prepared by dissolving 0.10 mol of NH4CH3COO in 0.500Lof 0.40 M HC2H3O2. Ka=1.8*10^-5 please show work
Calculate the pH of a solution prepared by dissolving 0.370 mol of formic acid HCOOH and 0.230 mol of sodium formate HCOONa in water sufficient to yield 1.00 L of solution. The Ka of formic acid is 1.77x10. -4 Seleccione una: a. 10.463 b. 2.307 O O c. 2.099 d. 3.546 e. 3.952
Calculate the pH of a solution that is prepared by dissolving 0.740 mol of hypochlorous acid (HCIO, Ka = 3.00x10-8) and 0.254 mol of hydrofluoric acid (HF, K, = 6.60*10-4) in water and diluting to 4.50 L. Also, calculate the equilibrium concentrations of HCIO, CIO-, HF, and F. Do not make an approximation unless the initial acid concentration is greater than 1000 ~ Kg. (Hint: The pH will be determined by the stronger acid of this pair.) pH = [HCIO]...
QUESTION 14 Calculate the pH of a solution prepared by dissolving 0.270 mol of formic acid (HCO2H) and 0.230 mol of sodium formate (NaCO2H) in water sufficient to yield 1.00 L of solution. The Ka of formic acid is 1.77X104 Enter your answer with three decimal places.
i need help with 6 b) please
6. a) Calculate the pH of a solution prepared by dissolving 0.0775 mol acetic acid and 0.0460 mol sodium acetate in 1 L of water. (Ka = 1.8 x 10-5) ANSWER: 4.52 b) Calculate the pH of the above solution if 0.0100 mol of KOH is added to this solution. ANSWER: 4.66