Phosphoric acid, H₂PO4 (aq), is a triprotic acid, meaning that one molecule of the acid has three acidic protons. Estimate the pH and the concentrations of all species in a 0.250 M phosphoric acid solution. [H₂PO4] = [H₂PO4] = [HPO2] = [PO] = x10 TOOLS M M M M pKal pK₂2 рКаз 2.16 7.21 12.32 [H+] = [OH-] = pH = M M

Phosphoric acid, H₂PO4 (aq), is a triprotic acid, meaning that one molecule of the acid has three acidic protons. Estimate the pH and the concentrations of all species in a 0.250 M phosphoric acid solution. [H₂PO4] = [H₂PO4] = [HPO2] = [PO] = x10 TOOLS M M M M pKal pK₂2 рКаз 2.16 7.21 12.32 [H+] = [OH-] = pH = M M

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

What is the pH of a 0.200 M solution of ammonium chloride (NH4Cl) Refer to these equations NH3(aq) + H2O(l) <=> OH-(aq) + NH4+(aq) Kb = 1.8 x 10-5 NH4+(aq) + H2O(l) <=> H3O+(aq) + NH3(aq) Ka = 5.6 x 10-10 5.44 4.98 3.44 1.66 2.70 8.91 7.23 9.00
The pH of a solution is a measure of the molar concentration of hydrogen ions, HO in moles per liter, in the solution, which means that it is a measure of the acidity or basicity of the solution. The letters pH stand for "power of hydrogen," and the numerical value is defined as pH =- log o[H] 10 Very acidic corresponds to pH values near 1, neutral corresponds to a pH near 7 (pure water), and very basic corresponds to values near 14. Rainwater is found to be slightly acidic compared to pure water. It has a hydrogen concentration of :10-5.6 What is the pH level of rainwater? A 1.2 5.6 6.2 (D 4.4
At the same concentration, which of the following aqueous solutions has the lowest pH? OHNO3 Sr(OH)2 O C6H5COOH (Ka = 6.3 x 10-5) O H2O NH3 (Kb = 1.8 x 10-5)
Calculate the percent ionization of a 1.00 M solution of hydrocyanic acid, HCN. Calculate the hydronium ion concentration of a solution containing 0.200 mol of HC₂H3O2 in 1.00 L of solution. K₂ = 1.80 × 10-5. What is the percent ionization of the acid?
The pH of a 8.3×10-2-M solution of phthalic acid (H2C8H4O4) is measured to be 2.03. Use this information to determine a value of Ka for phthalic acid. H2C8H4O4 (aq) + H 2 O(l) HC8H4O4- (aq) + H 3 O + (aq) K a =
For the diprotic weak acid H2A, ?a1=2.9×10−6 and ?a2=8.2×10−9. What is the pH of a 0.0650 M solution of H2A? pH= What are the equilibrium concentrations of H2A and A2− in this solution? [H2A]= M [A2−]=
Consider the following data on some weak acids and weak bases: name acid hydrocyanic acid nitrous acid solution 0.1 M KCN 0.1 M HONH3Br 0.1 M NaNO2 0.1 M KBr formula HCN HNO2 Ka 4.9 × 10 4.5 x 10 X - 10 PH choose one ✓ Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. choose one ✓ choose one choose one name S base formula hydroxylamine HONH₂ ethylamine C₂H5NH₂ | K₂ 1.1 × 10 6.4 × 10 8 4
A solution is made by dissolving 15.1 g of CH₃NH₃NO₃ in 500.0 mL of water. Using Ka(CH₃NH₃⁺) = 2.3 × 10⁻¹¹, determine the pH of the solution.
Calculating the pH of a strong base solution 1/5 A chemist dissolves 706. mg of pure potassium hydroxide in enough water to make up 50. mL of solution. Calculate the pH of the solution. (The temperature of the solution is 25 °C.) Round your answer to 2 significant decimal places. ப ☐ x10 ☑
Define pH in words. The strong acid HClaq has a pH value of 1, use the following equation for a strong acid: HClaq à H+aq + Cl-aq and convert the following expression to deduce the hydrogen ion concentration: pH = -log10 [H+] (ii) Use the above expression to deduce the pH of HCl (aq) given the concentration of the acid to be 4.5 mol/dm3
29.
1 being the lowest and 4 being the highest