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if a 0.076 M solution of chromic acid - 12 hours 24/48 pH-5.0510 Content attribution CONTENT...
Perform calculations for polyprotic acids Question Determine the concentration of Croa in a 0.031 M solution of chromic acid, H, CrO4. H,CrO4(aq) + H20(I) = H30+(aq) + HCrO] (aq) Ka = 9.6 HCrO2 (aq) + H2O(l) = H30+(aq) + Cro2- (aq) Kaz = 3.2 x 10-7 Report your answer in scientific notation with the correct number of significant figures. Provide your answer below:
The pH of a 0.13-M solution of arsenic acid (H3AsO4) is measured to be 1.65. Use this information to determine a value of K, for arsenic acid H3ASO4(aq)H20()H2AsO4(aq + H30*(aq)
The pH of a 0.23 M solution of acid HA is found to be 3.87. What is the Ka of the acid? The equation described by the Ka value is HA(aq) + H2O(l) <=> A-(aq) + H3O+ (aq) • Report your answer with two significant figures. Provide your answer below: K=0
Due Sunday, Nov 4, 11:59pm EST 9 Calculate pH During Acid Base Titration CONTENT FEEDBACK Question If 37.5 mL of 0.100 M NaOH is added to 10.0 mL of 0.100 M CH,COOH what will be the pH of the resulting solution? CHCOOHaą) + OH (aq) CH,CO (aq) + H,OU) Round your answer to three decimal places. Provide your answer below pi- MORE INSTRUCTION SUBMIT Content attribution
5. A 3.5 L sample of a 5.8 M NaCl solution is diluted to 55L. What is the molarity of the diluted solution? 6. Consider the reaction: K Slaq) + Co(NO3)2 (aq) → 2KNO3(aq) + Cos) What volume of 0.225 M K S solution is required to completely react with 175 mL of 0.115 M CO(NO3)2? 7. For each reaction, identify the Bronsted-Lowry acid, the Bronsted-Lowry base, the conjugate acid and the conjugate base a. Hl(aq) + H2O → H30*...
Calculate ka or kb from experimental data. The pH of a 8.7x10-2-M solution of maleic acid (H,C H204) is measured to be 1.52. Use this information to determine a value of K, for maleic acid. H2C4H204(aq) + H2O(1) P HC4H204 (aq) +H30*(aq) Ka=
The weak acid HIO has a Ka of 2.0×10−11. If a 1.7 M solution of the acid is prepared, what is the pH of the solution? The equilibrium expression is: HIO(aq)+H2O(l)⇋H3O+(aq)+IO−(aq) Report your answer with two significant figures.
Predicting pH Imagine you have a 0.125 M aqueous solution of aspirin, an acid drug with pKa = 3.5, in equilibrium. a) Estimate the pH of the solution Hint: Determine if it is an acid or base solution, weak or strong If weak acid/base, first try (H+) = /K,C, or [OH-] = K,C, b) Predict what would happen to the pH when you add more H2 Hint: First figure out what happens to the concentrations HA(aq) + H2O(0) A (aq)...
Data Table 1 Solution A.05M Acetic Acid IA (aq) + 1,0 (1) PH : 2.90 1,0' (aq) + (aq) 15 Molarity - Initial Concentration Change quilibrium Concentration 05-x K = [H,01[A] = [x][x] [HA] [.05-x] % ionization = [H0+1*100 [HA Jinitial = [x] * 100 .05 Data Table 2 Solution B 0.025M Acetic Acid PH: 3.00 IA (aq) + 10 (1) 1:0 (aq) + (aq) 1.025 Tolarity - Initial Concentration Change Equilibrium Concentration 1.025-X K = [x][x] [0.025-x] % ionization...
The pH of a 11.1 M solution of acid H, CO2 is found to be 2.660. What is the Ka of the acid? The equation described by the Ka value is H2CO (aq) + H2O)<HCO (a HO (aq) Report your answer with three significant figures