Find the pH of each mixture of acids given the table of Ka values.
7.5×10−2 M in HNO3 and 0.170 M in HC7H5O2
Ka for benzoic acid: is 6.5*10^-5
Thank you ?
All the best.
Find the pH of each mixture of acids given the table of Ka values. 7.5×10−2 M...
Find the pH of each of the following solutions of mixtures of acids. 8.0×10−2 M in HNO3 and 0.165 M in HC7H5O2, 1.5×10−2 M in HBr and 2.0×10−2 M in HClO4, 9.5×10−2 M in HF and 0.230 M in HC6H5O, 0.110 M in formic acid and 4.5×10−2 M in hypochlorous acid PLEASE show work
pH of Weak Acids 19. Consider the following acids; CH5COOH ( benzoic acid) Ka = 6.14x10-5 H3BO3 (boric acid) Ka = 5.83x10-10 H2P04 (dihydrogen phosphate) Ka = 6.30x10-8 HNO3 (nitric acid) >>> 1 Put the acids in order from strongest to weakest. 20. Calculate the pH and percent ionization of the following solutions (Use ICE for weak acid calculation) a. 0.15 M HNO3 0.82; 100% b. 0.15 M HNO2 ( ka = 4.5x10-5) 2.59; 1.71%
Assuming 0.1 M concentrations, arrange the following acids in order of increasing pH. benzoic acid, HC7H5O2, Ka ≡ 6.3 × 10−5 chlorous acid, HClO2, Ka ≡ 1.1 × 10−2 formic acid, HCHO2, Ka ≡ 1.8 × 10−4 hydrofluoric acid, HF, Ka ≡ 6.8 × 10−4
Calculate the pH at the equivalence point in titrating 0.047 M solutions of each of the following with 0.055 M NaOH. (a) nitric acid (HNO3) pH = (b) acetic acid (HC2H3O2), Ka = 1.8e-05 pH = (c) benzoic acid (HC7H5O2), Ka = 6.3e-05 pH = Calculate the pH at the equivalence point in titrating 0.047 M solutions of each of the following with 0.055 M NaOH. (a) nitric acid (HNO3) pH = (b) acetic acid (HC2H302), Ka = 1.84-05...
Calculate the pH at the equivalence point in titrating 0.047 M solutions of each of the following with 0.055 M NaOH. (a) nitric acid (HNO3) pH = (b) acetic acid (HC2H3O2), Ka = 1.8e-05 pH = (c) benzoic acid (HC7H5O2), Ka = 6.3e-05 pH = Calculate the pH at the equivalence point in titrating 0.047 M solutions of each of the following with 0.055 M NaOH (a) nitric acid (HNO3) pH= (b) аcetic acid (HC2H302), ка = 1.8e-05 pH =...
Calculate the pH at the equivalence point in titrating 0.028 M solutions of each of the following with 0.031 M NaOH. (a) nitric acid (HNO3) pH = ______ (b) benzoic acid (HC7H5O2), Ka = 6.3e-05 pH = _______ (c) hypobromous acid (HBrO), Ka = 2.5e-09 pH = _______
Find the pH of each of the following solutions of mixtures of acids. No Ka is given. Part A.) 0.125 M in HBr and 0.145 M in HCHO2 (Gave up, Answer pH= 0.903) Part B.) 0.145 M in HNO2 and 9.0×10−2 M in HNO3 Part C.) 0.190 M in HCHO2 and 0.23 M in HC2H3O2
Finding ph in a mixture of weak acids. Please explain:) Mixture of weak Acids: Find the pH of a mixture that is 0.150 M HF and 0.100 M HCIO. Ka of HF 3.5 x 10-4 K, of HCIO 2.9 x 10 Kw of H20 1.0 x 10-14 In a mixture of 2 weak acids in which one is weaker than the other, the H contribution from the ionization of the weaker acid can be ignored in calculating the pH of...
Calculate the pH and percent dissociation of 1.12 M benzoic acid, HC7H5O2, Ka = 6.3 × 10–5
calculate the pH of a 0.30 M solution of benzoic acid (HC7H5O2, Ka = 6.5x10-5)