The value of Ka for acetylsalicylic acid (aspirin), HC9H704, is 3.00×10-4. Write the equation for the reaction that goes with this equilibrium constant. (Use H3O+ instead of H*.) = + +
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- The pigment cyanidin aglycone is one of the anthocyanin molecules that gives red cabbage (Brassica oleracea var. capitata f. rubra) its characteristic red coloration. Many chemistry students have used this red cabbage indicator to study acid-base chemistry. Estimate tire pH range at which cyanidin agly-cone shows a color change. Anth-H(aq) Anth(aq) + H+ (aq) Ka = 1.3 107Formic acid dissociates reversibly according to the following equation. [ /20] HCOOH(aq) ⇌ HCOO-(aq) + H+(aq) Write the law of mass action for this equilibrium.K = Is the equilibrium constant in (a) a Ka? Briefly explain. If a solution is initially 0.20 mol/L HCOOH and the equilibrium constant in (a) is 1.8 × 10-4, what is the concentration of hydrogen ions at equilibrium? Show your work. Use the value obtained in (c) to find the solution’s pH and pOH at 25 °C. If you were unable to complete (c), you may assume a 0.0030 mol/L concentration of hydrogen ions. Would the addition of sodium formate (NaHCOO) to this solution increase pH? Explain.Determine the Ka for an acid by constructing an ICE table and using this information to construct and solve the equilibrium constant expression. Complete Parts 1-2 before submitting your answer. NEXT > The pH for 0.0850 M solution of C6H5CH₂COOH is 2.68. Fill in the ICE table with the appropriate value for each involved species to determine the unknown concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) -0.0829 C6H5CH₂COOH(aq) + 0 1 0.428 0.0850 -0.428 2.68 H₂O(l) -2.68 = 2 HgO+(aq) 2.1 x 10-³ + C6H5CH₂COO-(aq) -2.1 x 10-3 RESET 0.0829
- Consider the following chemical equilibrium: HCOO¯¯ (aq) + H₂O(aq) = HCOOH(aq) + OH¯(aq). Which of the following graphs represents the perturbation on the system and the change of pH when HCI is added to the container? | pH time || III pH ↑ time Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. C Q a || = III = d IV pH IV pH time time K Open Χ Your answeraching and lea x A My Drive- Google Drive now.com/ilrn/takeAssignment/takeCovalentActivity.do?locator=Dassignment-take [Review Topics] [References] Use the References to access important values if needed for this question. The value of K, for acetic acid , CH,COOH, is 1.80×10. Write the equation for the reaction that goes with this equilibrium constant. (Use H30 instead of H.) Submit Answer Retry Entire Group 9 more group attempts remaining hpConsider the following acid-base reaction: H3O+ + HPO42 H₂PO4 + H₂O Identify the Bronsted-Lowry base. OH₂O ⒸHPO4 ²- OH₂PO4 OH3O+ What is the concentration (in Molarity) of a Sulfuric Acid (H₂SO4) solution if a 15.0 mL sample required 26.4 mL of 0.950 M KOH for neutralization? H₂SO4 + 2 KOH --> K₂SO4 + 2 H₂O (balanced) 0.012 M 0.025 M 0.836 M 0.270 M
- Consider the reaction below. What is the effect on the concentration of ammonia (NH3 ), water (H20) hydroxide ion (OH"), and ammonium ion (NH+) if OH is added to the reaction? NH3 (aq) + H2O (1) = NH4* (aq) + OH (aq) K-1.8x1Q-5 The concentration of NH3 The concentration of OH- The concentration of NHA+ The concentration of H2 increases decreases does not changeOne way to determine the predominant species at equilibrium for an acid-base reaction is to say that the reaction arrow points to the acid with the higher value of pK. For example, NH, + H,0 NH, + H,O+ pK. pk, 9.24 pK-1.74 NH,+ + OH--→ NH, + H,0 рк, 9.24 pK, 15.7 Explain why this rule works.The pH of a 0.0200 M solution of an unknown acid is 2.56. What is the Ka of this acid? To solve this problem: Write the acid dissociation equilibrium for the generic acid “HA” Set up an ICE chart ( with x = the concentration of H3O+ at equilibrium) Write the expression for Ka. Fill this in with the concentrations of H3O+, A- and HA at equilibrium, in terms of x. What is x? Can you find it from the given information? You should be able to use the pH to get the concentration of H3O+, which is x. Do this. Now that you know x, plug in into the Ka expression and find Ka.
- Determine the Ka for an acid by constructing an ICE table and using this information to construct and solve the equilibrium constant expression. Complete Parts 1-2 before submitting your answer. 1 2 NEXT The pH for 0.0715 M solution of CC13CO2H is 1.40. Fill in the ICE table with the appropriate value for each involved species to determine the unknown concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) -0.032 CCI CO₂H(aq) + H₂O(1) H3O+(aq) + CCI CO₂-(aq) RESET 0 0.0715 1.40 -1.40 0.040 -0.040 0.032Which of the following expressions is the correct equilibrium-constant expression for the reaction below? HF (aq) + H2O (l) H3O+ (aq) + F- (aq) Group of answer choices [H3O+][F-] / [HF] [F-] / [HF] [HF][H2O] / [H3O+][F-] [H3O+][F-] / [HF][H2O] 1 / [HF]Determine the pH of a solution of aspirin (acetylsalicylic acid, HC,H,O4) by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. The Ka of aspirin is 3.3 x 10-4. Complete Parts 1-3 before submitting your answer. Initial (M) Change (M) Equilibrium (M) -X NEXT > 652 mg of aspirin (HC9H₂O4) is dissolved in an aqueous solution of 237 mL aqueous solution. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. 15.3 - x 0 1 HCgH;O4(aq) 2.75 x 10-3+x 0.0153 + x 2.75 x 10-3 2.75 x 10-3-X 0.0153 - x + 2 H₂O(1) 3.62 x 10-³ 3.62 x 10-3+x = 1.53 x 10-5 3.62 x 10-3-x 3 H3O+ (aq) 15.3 1.53 x 10-5 + x 0.0153 + 1.53 x 10-5-x C9H₂O4 (aq) RESET +X 15.3 + x