Initial (M) Change (M) Equilibrium (M) -X 15.3 - x 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. Complete Parts 1-3 before submitting your answer. 0 652 mg of aspirin (HC,H,O4) 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. 1 HC,H,O,(aq) 2.75 x 10-³ + x 0.0153 + x 2.75 x 10-³ 2.75 x 10-³-: Question 23 of 26 0.0153 - x + 2 H₂O(1) 3.62 x 10-³ 3.62 x 10-³ + x = 1.53 x 10-5 3 3.62 x 10-³ - x H,O*(aq) 15.3 1.53 x 10-5 + x NEXT > 0.0153 + 1.53 x 10 x C₂H₂O4 (aq) RESET +x 15.3 + x

7:30 1 y gmail x H Folde x A FINAL X E Prese x Prese x E PRESE X * Ceno x Y short x RI Anno x w weba x y chem x à app.101edu.co Time's Up! Write the acidic equilibrium equation for CH.NH:. 1 3 4 5 6 8 9 Os + (s) (1) (g) (ag) HO OH H:O H Reset • x H:O Delete (0) 7°C Mostly doudy a O od0 ENG P Type here to search

Construct the expression for Ka for the weak acid, HCSH-O4. HC-H-O:(aq) + H2O(I) = H:O*(aq) + C»H;Os (aq) 1 Based on the definition of Ka, drag the tiles to construct the expression for the given acid. Ка RESET [H:O] [H.O*] [OH] [HC-H.O:] [H:C»H÷O.] [CH:O.] 2[H:O] 2[HO*] 2[OH] 2[HCH.O:] 2[H:C»H-O.*] 2[CH-O.] [H:O]? [H.O*j? [OH-P [HC»H-O.JP [H:CH.O.*]? [CH:O.?

Aspirin (acetylsalicylic acid, C9H3O4) is a weak monoprotic acid. To determine its acid-dissociation constant, a student dissolved 2.00 g of aspirin in 0.600 L of water and measured the pH. What was the Ka value calculated by the student if the pH of the solution was 2.61? Express your answer numerically using two significant figures. • View Available Hint(s) ? Ka =

pH - 10.5 pOH - 3.3 Equilibrium [OH–] -  Equilibrium [Mg2+] -  Molar Solubility -  Ksp -  I Need Help Finding Out The Rest Please !

For different enzymes, there is an optimum pH at which the enzyme is most active. For example, for enzymes of gastric juice optimum pH 1-2, for duodenal enzymes pH 7.7, for liver enzymes pH 9.5, etc. Determine which medium (a or b) is most favorable for each of the enzymes mentioned above if the following substances are added to 1.0 liter of water: a) 0.040 mol KOH and 0.030 mol HBr; b) 4.0 10-9 mol HNO3. Neglect the change in the volume of the solution. Confirm your answer with calculations.

i hope that you can answer both please

An acid (HA) dissociates as follows: HA → H* + A minus Arrow should be interpreted as an equilibrium arrow. The pH of the 0.15 M solution of HA is 4.31. What is [H*]? Express your answer as a decimal, not an exponent. Please include a proper (abbreviated) unit. Your Answer: Answer units

We dissolve 0.661 mol of a weak acid, HA, and 13.7 g of NaOH in enough water to produce 1.00 L of solution. The final pH of this solution is 4.54. What is the dissociation constant, Ka, of HA? The temperature is 25.0°C. Your Answer: Answer

An acid (HA) dissociates as follows: НА - H* + A minus Arrow should be interpreted as an equilibrium arrow. The pH of the 0.85 M solution of HA is 1.35. What is the K, of HA? Express your answer as a decimal, not an exponent. No unit, please. Your Answer: Answer