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![[H2O2 (aq)],
M
0.0850
0.170
0.250
0.350
0.350
0.350
0.350
[l* (aq)], M
0.100
0.100
0.100
0.100
0.200
0.300
0.400
A [H₂O₂ (aq)]
At
1.4
2.9
4.2
5.9
12
18
24
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- Phosphoric acid, H3PO4(aq),H3PO4(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 0.150 M phosphoric acid solution. pKa1= 2.16 pKa2= 7.21 pKa3= 12.32 [H3PO4]= ? M [H2PO−4]= ? M [HPO2−4]= ? M [PO3−4]= ? M [H+]= ? M [OH−]= ? M pH=Phosphoric acid, H3PO4(aq),H3PO4(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 0.400 M phosphoric acid solution. pKa1: 2.167 pKa2: 7.21 pKa3: 12.32Calculate K₂ or K from experimental data. The pH of a 0.14-M solution of chlorous acid (HCIO₂) is measured to be 1.49. Use this information to determine a value of Ka for chlorous acid. HCIO₂(aq) + H₂O(l)=CIO₂ (aq) + H₂O˚(aq) K₂ =
- HN3(aq) + H2O(l) ⇌ N3-(aq) + H3O(aq) Calculate the hydronium ion concentration and pH of a 0.045 M solution of chloroacetic acid. (Ka = 1.3 x 10-3). Chloroacetic acid is a monoprotic acid, i.e. it reacts with water in a 1:1 mole ratio.10. Calculate the pH of a solution of CH3NH2(aq) Methylamine, Kb = 4.3x104 that has an initial concentration of 0.20 M? Is it acidic, basic, or neutral solution?In the following equation HNO2 (aq) + H2O (l) ↔ H3O+ (aq) + NO2-(aq), 0.37 M of nitrous acid was found in the resulting aqueous solution. If Ka for HNO2 is 4.5 x10 -4, what is the pH of the HNO2 solution? 1.75 1.78 1.88 1.9
- Calculate the concentration of H3O+ in a solution that contains 4.4 × 10–6 mol L–1 OH– at 25 °C. Also identify the solution as acidic, basic, or neutral. 2.1 × 10–3 mol L–1, basic 2.3 × 10–9 mol L–1, acidic 2.1 × 10–3 mol L–1, acidic 2.3 × 10–9 mol L–1, basic 4.4 × 10–6 mol L–1, neutral2a. Consider the reaction: H₂O(1) H*(aq) + OH(aq), which is known at the autoionization of water. Using data from the table below, calculate AH° and AS° for the autoionization of water. T(°C) pKw 0 14.94 14.00 25 35 13.68 13.53 40 50 13.26Predict the product of SO3(g)+2H2O(l) and whether the solution at equilibrium will be acidic, basic, or neutral.
- What is the pH of .76 M CN (aq)? O 13.9 O 4.7 O 9.3 O 2.4 O 11.63. A 0.0560 g quantity of acetic acid is dissolved in enough water to make 50.0 mL of solution. Calculate the concentrations of H;O*, CH;COO and CH;COOH at equilibrium. What is the pH of the solution? (Ka = 1.8x10) CH;COOH(aq) = CH;COO (aq) + H;O* (aq) a) Calculate the initial concentration of CH;COOH. (C:12; H:1; 0:16) b) Calculate the concentration of CH;CoO (aq) and H;O* (aq) at equilibrium. c) Calculate pH of the solution.Nitrous acid, HNO2 (aq) has a Ka value of 4.0 x 10-4. What is the pH and POH of a 0.0500 M solution of lithium nitrite? (Assumptions may not be valid.)