Write a net ionic equation for the overall reaction that occurs when aqueous solutions of ascorbic acid (H,C,H,O) and sodium hydroxide are combined. Assume excess base. Be sure to specify states such as (aq) or (s).
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- A weak acid has a Ka of 7.6 x 106. What is the value of pk for the acid? a pKa =Given the following information: nitrous acid HNO2 hydrocyanic acid = HCN HNO, is a stronger acid than HCN (1) Write the net ionic equation for the reaction that occurs when equal volumes of 0.058 M aqueous nitrous acid and sodium cyanide are mixed. It is not necessary to include states such as (aq) or (s). (2) Which is the strongest base, NO, or CN ? (3) At equilibrium the will be favored.3. 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.
- Write a net ionic equation for the overall reaction that occurs when aqueous solutions of potassium hydroxide and oxalic acid (H₂C₂O4) are combined. Assume excess base. Be sure to specify states such as (aq) or (s). + +Given the following information: nitrous acid = HNO, = CH,COOH acetic acid HNO, is a stronger acid than CH;COOH (1) Write the net ionic equabon for the reaction that occurs when equal volumes of 0.070 M aqueous nitrous acid and sodium acetate are mixed it is not necessany to include states such as (aq) or (8) (2) Which is the strongest base, NO, or CH,CO0 ? (3) At equilibrum the will be favored.(i) 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
- (i) 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 pH =Propanoic acid, CH₂CH₂COOH, is a weak monoprotic acid that is used to inhibit mould formation in bread. A student prepared a 0.10 mol/L solution of propanoic acid and found that the pH was 2.96. What is the acid dissociation constant for propanoic acid? [Hint: Setup an I.C.E. table] CH3CH₂COOH (aq) Ka for propanoic acid is: ←CH3CH₂COO (aq) + H (aq)Calculate the equilibrium constant for the following reaction: CH3COOH(aq) + F¯ (aq)=CH₂COO (aq) + HF (aq) Be sure your answer has the correct number of significant digits. Note: Reference the K of acids at 25 °C table for additional information. a x10 x S
- At 50 °C, the ion-product constant for H2O has the valueKw = 5.48 x 10-14. (a) What is the pH of pure water at50 °C? (b) Based on the change in Kw with temperature,predict whether ΔH is positive, negative, or zero for theautoionization reaction of water:2 H2O(l) ⇌ H3O+(aq) + OH-(aq)For the following acid-base reaction, (1) predict the products, showing both reactants and products complete Lewis structures and arrows showing electron flow; (2) label each structure with the lowing: Bronsted acid, Bronsted base, conjugate acid, conjugate base; (3) give a brief definition of a ronsted acid and Bronsted base; (4) predict the direction of the equilibrium and justify your answer. HC0OH + CH3 Nta PRん106Y pkb = 3.36Calculate the pH and PO, concentration in 2.25 M phosphoric acid (H;PO.) solution? H3PO,(aq) + H2O(1) = H;O^(aq) + H,PO, (aq) Ka1 = 7.1×10 H2PO, (aq) + H,O(1) = H,O*(aq) + HPO,² (aq) K, 2 = 6.3×10¯ HPO (aq) + H,O(1) = H;O*(aq) + PO," (aq) K,3 = 4.2×101³ O a. pH = 0.948; [PO,"] = 2.38×10 *° M. on O b. pH = 0.875; [PO,"] = 1.99×10¬1º M Oc pH = 0.986; [PO, 1 = 2.56×10¬1ª M O d. pH = 0.924; [PO,"] = 2.22×10¬1° M O e. pH = 0.898; [PO,1 = 2.09×10 1º M