Butyric acid, CH3CH₂CH₂CH₂COOH, is a weak acid. It ionises in water to produce butanoate and hydronium ions. Select the correct balanced equation for the ionisation of butyric acid: Select one: a. CH3CH₂CH₂COOH CH3CH₂CH₂COO b. CH3CH₂CH₂COO + H₂0+ ⇒ CH3CH₂CH₂COOH + H₂O C. CH3CH₂CH₂COOH ⇒ CH3CH₂CH₂Cоо¯ + H₂O+ O d. CH3CH₂CH₂COOH + H₂O ⇒ CH₂CH₂CH₂COO + H3O+

Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the appropriate equilibrium equation for the acid or base that exists when the salt is dissolved in aqueous solution. If neutral, simply write only NR. CSHSNHI 04- D2+ 3+ 4+ 1 2 4 5 7 9 3 Os (s) (1) (g) (aq) + OH- NR H H3O+ C H2O Reset • x H2O Delete CO LO

Calculate the concentration of an HCl solution if 100.0 mL of the HCI required 33.00 mL of 0.2000 M Mg(OH)₂ to reach the titration endpoint. Mg(OH)2 + 2 HCl → 2 H₂O + MgCl₂ There is enough information to calculate the moles of base but not the moles of acid. mol b. 0.1320 i. OH-1 p. CO3² W. PO4³ a. 0.1000 h. CaCO3(s) o. H₂PO4-¹ v. H₂CO3 bb. 3.300 x 10-² hh. 2.16 x 10-6 L)(- mol Mg(OH)3)(- mol HCI c. HX j. H30+1 q. HCO3-¹ x. HCzH3Oz dd. 2 jj. 0.2000 d. Al+3 k. SO4² r. H₂S CC. 3 ii. 1.60 x 10-5 e. CO₂ 1. Mg+2 S. HS-1 y. C₂H30₂-1 ee. 1 = mol HCI mol Mg(OH)₂ M HCI f. CaF2(aq) m. C-1 t. S-2 z. 1 x 10-14 ff. 0.099536 kk. 6.600 x 10-³ g. HF(aq) n. HPO 2 u. H₂O(lig) mol Mg(OH)3 aa. 1.32 x 102 gg. 3.95 x 10-3 mol HCI

HO -OH Oxalic Acid, H₂C₂O₁ PK₁₁ = 1.27 pka2 = 4.266 H₂Ox→ HOX → Ox ²- H₂A → HA → A²- pH = ? Adding 0.20 mole of NaOH to 0.40 mole of NaHC₂O4 (s) with total volume of 500 mL. pH = ? 150 g of NaHC₂O4 (s) dissolved in DI water total volume of 500 mL. pH = ? Adding 0.20 mole of HCI to 0.40 mole of NaHC₂O4 (s) with total volume of 500 mL. pH = ? 0.40 Adding 0.20 mole of HCI mole of Na₂C₂O4 (s) with total volume of 500 mL. pH = ? Adding 0.40 mole of HCI to 0.40 mole of Na₂C₂O4 (s) with total volume of 500 mL. pH = ? Important Key Concept Exercise