* Vinegar - colour of solution = bright pink, observed pH = 1, Measured pH = 1.62 *Soap - colour of solution purple, observed pH = 6, Measured pH = 5.60 *Laundry Detergent - colour of solution blue green, observed pH 10, = I Measured pH = 8.20 A. Show your calculation for [H30 +] and [OH-] values for each product and indicate if it is an acidic or a basic substance. (20p) Skip question Exit Tyne here to search

* Vinegar - colour of solution = bright pink, observed pH = 1, Measured pH = 1.62 Soap - colour of solution purple, observed pH = 6, Measured pH = 5.60 Laundry Detergent - colour of solution blue green, observed pH 10, = I Measured pH = 8.20 A. Show your calculation for [H30 +] and [OH-] values for each product and indicate if it is an acidic or a basic substance. (20p) Skip question Exit Tyne here to search

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Calculate the pH and the concentration of all the species present at equilibrium for a 1.0E-4 M asorbic acid H2C6H6O6 solution. pKa1 = 4.1; pKa2 11.8
2. Answer the questions for the acid below: HA(aq) + H20(l)→H30+(aq) + A-(aq) a) Write the acid dissociation constant, Ka, expression for the reaction: b) If [A] = 0.030 M, [H3O*] = 0.010 M, and [HA] = 0.5 M, what is the value of Ka? %3D c) If another acid, HB, has a Ka value of 1.0 x 10-10, which acid is stronger? HA or HB? Why?
Please help balanced these reactions. NaOH (aq) + CuSoH & Cu (OH)2 (5) + Na2504 (aq) Naci (aq) + agwo3 (aq) à Agc1 (6) +N (IND3 (09) Naz ((0)3 (99) + HCl(aq) -> Baso4 (6) + HCl (69) (1/a) (66)3 (69)+ HC (99)-) (02 (g) + H₂0 + Naot lag)+ HC (aq) -> H₂0 (1) +rack (aq) zn (5) + H2 SO4 (99) -) 2n504 (ag) + H2 (g) mg (5) + HCl(aq). -> H+2 (g) + mgc12 (69) 20/5) + (US04 (04) -> (u (5) + Zn S04 (09)
If two water samples were collected as follows: Sample #1 with a pH = 8.8 and the concentration of [HCO3-] = 0.01 molar Sample #2 with a pH = 87.0 and the concentration of [HCO3-] = 0.00 molar Compare the alkalinity of the two samples Which of these two samples was taken from a well-buffered lake?
Calculate the pH and the equilibrium concentrations of H₂PO4, HPO42- and PO4³- in a 0.0960 M aqueous phosphoric acid solution. For H3PO4, Ka1 = 7.5x10-3, Ka2 = 6.2x10-8, and Ka3 = 3.6x10-13 pH = [H₂PO4] = [HPO4²-] = [PO4³-] = 3 M M
Calculate the pH at 25 °C of a 0.20M solution of potassium butanoate (KC,H,CO,). Note that butanoic acid (HC,H,CO,) is a weak acid with a pK, of 4.82 Round your answer to 1 decimal place. pH = ?
Calculate the pH at 25 °C of a 0.98M solution of sodium propionate (NaC₂H-CO₂). Note that propionic acid (HC₂H₂CO₂) is a weak acid with a p K of 4.89. a Round your answer to 1 decimal place. -0 pH = X S
Calculate the pH at 25 °C of a 0.87M solution of potassium butanoate (KC,H,CO,). Note that butanoic acid (HC;H,CO,) is a weak acid with a p K, of 4.82. Round your answer to 1 decimal place. pH = 0 ? alo 18 Ar
What is the pH of rainwater in equilibrium with 0.531 ppm SO₂ (KH = 1.0 M-atm 1) when sulfurous acid is the only source of acidity and no further oxidation has taken place? (K₂ sulfurous acid = 1.7 x 10-²) O4.02 O 7.15 5.58 O 6.03 O 5.04
pH 124 14 12 10 4 2 0 10 20 30 40 50 Volume (ml) Identify the weak acid according to the pH curve shown. A. Chloroacetic Acid; Ka = 1.4 x 10-³ B. Hydrogen Phosphate; Ka = 2.2 x 10-¹3 C. Hypobromous Acid; Ka = 2.0 x 10-⁹ - D. Hydrazoic Acid; Ka = 1.9 x 10-5
at What is the principle form of a triprotic acid (HSA) pH 8? What is the pH of a 0.500M Solution of на 2+? pkal = 1.99; pka₂ = 3.90 jpka z = 10.00
Selenic acid, H2SeO4, is a diprotic acid that actually is a strong acid for the donation of its first proton and has a pKa2 = 1.7. What will be the Ka and the chemical equation for showing the donation of the second proton? (hint: products will be H3O+ and SeO42-) I take 2.00 g the pure compound and dilute it to 100.0 mL of solution. Find the initial concentration and use two ICE tables to show the equilibrium concentrations of [H3O+], [OH-], [HSeO42-] and [SeO42-]. What will be the concentration of H2SeO4? (hint: no math is necessary here as this is a strong acid).