(a) 0.49 M cyanic acid (HCNO, PK₂ = 3.46) 0.02 X % The approximation is valid. O The approximation is not valid. (b) 0.0014 M hydrazoic acid (HN3, PK₂ = 4.6) % O The approximation is valid. The approximation is not valid. (c) 5.7 M arsenic acid (H3ASO4, PK₂ = 2.26) % The approximation is valid. O The approximation is not valid.
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- The pH reading of a sample of each substance is given. Calculate the hydrogen ion concentration of the substance. (Give your answers in scientific notation, correct to one decimal place.) (a) Vinegar: pH = 3 %3D [H+] = x 10 M (b) Crackers: pH = 7.2 %3D [H+] = x 10 M (p ツCOHSOH(ag) + H2On + CeHsO (aq) + H3O*(a9) Ka= 1.12 x 10-10 (a) Phenol is a weak acid that partially dissociates in water according to the equation above. Write the equilibrium-constant expression for the dissociation of the acid in water. (b) What is the pH of a 0.75 M CaHsOH(ag) solution? (C) For a certain reaction involving CaHsOH(ag) to proceed at a significant rate, the phenol must be primarily in its deprotonated form, C3H5O (eg). In order to ensure that the CsHsOH(aq) is deprotonated, the reaction must be conducted in a buffered solution. On the number scale below, circle each pH for which more than 50 percent of the phenol molecules are in the deprotonated form (CoHsO (aq). Justify your answer. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 Justification: (d) CeHsOH(ag) reacts with NaOH(ag). Write a net ionic equation representing this reaction (aka: invasion equation). (e) What is the pH of the resulting solution when 30 mL of 0.40 M CSH5OH(aq) is added to 25 mL of 0.60 M NAOH. Show all work…The chemical formulae of some acids are listed in the first column of the table below, and in the second column it says whether each acid is strong or weak. Complete the table. List the chemical formula of each species present at concentrations greater than about 106 mo mo-when about a tenth of a mole of the acid is L dissolved in a liter of water. The chemical formulae of some acids are listed in the first column of the table below, and in the second column it says whether each acid is strong or weak. Complete the table. List the chemical formula of each species present at concentrations greater than about 10-6 mol/L when about a tenth of a mole of the acid is dissolved in a liter of water. acid strong or weak? species present at 10-6 mol/L or greater when dissolved in water ICIO weak H₂SO, weak IICI strong HCIO, strong ☐ x DO....
- A student is provided with a 0.1 M stock solution of NaOH. Student was then asked to mix 50.0 mL of this stock solution of NaOH with 450.0 mL of water to prepare a dilute solution of NaOH. (A) Calculate the molarity of the diluted solution. (B). Calculate the hydronium ion concentration, [H3O+] in the final diluted solution. (8 points) (C ) Calculate the pH of the diluted NaOH solution. (D) Is the final diluted solution acidic, basic or neutral?Propionic acid, HC3H5O2, has Ka= 1.34 x 10–5. (a) What is the molar concentration of H3O+ in 0.15 M HC3H5O2 and the pH of the solution? (b) What is the Kb value for the propionate ion, C3H5O2–? (c) Calculate the pH of 0.15 M solution of sodium propionate, NaC3H5O2. (d) Calculate the pH of solution that contains 0.12 M HC3H5O2 and 0.25 M NaC3H5O2.Consider the reaction below. Co(H,O),* (aq) + 4 Cl¯ (aq) = COC1," (aq) + 6 H,O (1I) The equilibrium constant expression (K) of the reaction does not include the concentration of H,O even though the reaction produces six moles of water. Explain.
- Three acids found in foods are lactic acid, LA, (in milk products), oxalic acid, OA, (in rhubarb), and malic acid, MA (in apples). The pKa values are LA =3.88, OA =1.23, and MA =3.40. Which list has the conjugate bases of these acids, lactate, oxalate, and malate, in order of decreasing strength? O lactate > malate > oxalate lactate > oxalate > malate malate > lactate > oxalate oxalate > malate > lactateAcetic acid is a weak acid, meaning it does not fully dissociate in water. Instead, there is an equilibrium between the dissolved but undissociated molecule and the component ions: HOAc (aq) + H2O (l) ⇌ H3O+ (aq) + OAc– (aq)OAc– is an abbreviation for the acetate ion, CH3COO–, and H3O+ is the hydronium ion (lone protons, H+ (aq), do not exist!). (d) When starting with completely un-dissociated acetic acid, is it accurate to assume that [HOAc]0 = [HOAc]eq? Why or why not? (e) A highly concentrated acetic acid solution contains 15.0M acetic acid at equilibrium. What are the equilibrium concentrations of the hydronium and acetate ions in this solution? (f) Creating the concentrated acetic acid solution by dissolving liquid HOAc in water raises the temperature of the water by about 5°C from room temperature. At 50°C, do you expect the solution to contain more or less acetate ion OAc– than what you calculated in (c)? Why?Acetic acid is a weak acid, meaning it does not fully dissociate in water. Instead, there is an equilibrium between the dissolved but undissociated molecule and the component ions: HOAc (aq) + H2O (l) ⇌ H3O+ (aq) + OAc– (aq)OAc– is an abbreviation for the acetate ion, CH3COO–, and H3O+ is the hydronium ion (lone protons, H+ (aq), do not exist!). (a) Write the equilibrium constant expression for the dissociation of acetic acid. (b) Vinegar sold commercially is typically 0.8 − 1.0 M acetic acid. A 1.00 M solution of acetic acid is measured by its pH to have an equilibrium concentration of 4.19×10−3 M for both acetate ions and hydronium ions at room temperature. Assuming [HOAc]0 = 1.00M, what is the equilibrium concentration of undissociated acetic acid [HOAc]eq to the correct number of significant figures? (c) What is the value of the equilibrium constant Keq for the dissociation according to the concentrations from part (b)? (d) When starting with completely un-dissociated…
- Q3. This question is about the pH of several solutions. Give all values of pH to 2 decimal places. (a) (i) Write an expression for pH. (b) (ii) Calculate the pH of the solution formed when 10.0 cm³ of 0.154 mol dm-³ hydrochloric acid are added to 990 cm³ of water. The acid dissociation constant, Ka, for the weak acid HX has the value 4.83 x 10-5 mol dm-³ at 25 °C. A solution of HX has a pH of 2.48 Calculate the concentration of HX in the solution. Page 4 of 148. (a) Calculate the percent ionization of a 0.20 M solution of the monoprotic acetylsalicylic acid (aspirin) for which Ka = 3.0 x 10-4 .(b)The pH of gastric juice in the stomach of a certain individual is 1.00. After a few aspirin tablets have been swallowed, the concentration of acetylsalicylic acid in the stomach is 0.20M. Calculate the % ionization of the acid under these conditions. What effect does the nonionized acid have on the membranes lining of the stomach? 9. Calculate the [H+], [C2O4-2], and [H2C2O4] in a 0.0010M H2C2O4 solution. (Ka = 5.4 x 10-2)Suppose each circle below represents a container of an aqueous solution of three different acids, HA (Ka = 1 × 10−3), HB (Ka = 1 × 105), and HC (Ka = 1 × 10−8). Draw a representative particulate level diagram of all the predominant species, and their relative quantities, at equilibrium if the initial concentrations of all three solutions were the same. Omit water molecules for clarity.