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- i) CH;NH2 i) ii) LIAIH, ii) H,0Chemists working with fluorine and its compounds some- times find it helpful to think in terms of acid-base reac- tions in which the fluoride ion (F¯) is donated and ассеpted. (a) Would the acid in this system be the fluoride donor or fluoride acceptor? (b) Identify the acid and base in each of these reactions: CIF;O2 + BF; CIF,O, · BF, -- TiF, + 2 KF – K2[TiF,](f) Calculate the pH of the following solutions: (i) A 0.045 M solution of sulphuric acid. (ii) A solution containing 0.4 g sodium hydroxide in 100 cm³ water. (iii) Given the Ka value for CH3COOH is 1.8 x 10-5, calculate the pH of the acid. The initial concentration of the acid is 0.2 M
- The ionization constant of lactic acid, CH,CH(OH)CO,H, an acid found in the blood after strenuous exercise, is 1.36 x 10-4. What is the concentration of hydronium ion in the solution of 0.102 M lactic acid? CH;CH(OH)CO,H (aq) + H,O (1) → H;O• (aq) + CH;CH(OH)CO, (aq) O 0.00372 M O 0.0165 M O 0.00549 M O 0.227 MComplete the balanced chemical reaction for the following weak base with a strong acid. In this case, write the resulting acid and base as its own species in the reaction. CH;NH2(aq) + HCIO3(aq) > 4- 3. 2+ 3+ 4+ 1 2 6 7 8 O2 4 5. ) (s) (1) (g) (aq) H N H30* CI H20 OH 4- +i need the answer quickly
- What is the pH of a 0.660 M solution of C5H5NHB (Kb of C3H;N is 1.7 10-9)?(a) (1) CI AICI (2) HNO₂, H₂SO (3) O (4) Me,S (5) NaBH; H₂O+ एल Draw Your Solution3a. (2)A student prepared a 0.0750 M NaOH solution for a titration experiment. If it took 25.52 ml of the NaOH to turn the H2SO4 solution faint pink, how many moles of NaOH were required to reach the end point? 3b. (4)What was the mole of H2SO4 used from 3a. question?
- 4. (a) Calculate [H3O*] and [OH] for the solutions indicated: lemon juice, pH = 2.42 (1) (ii) household ammonia pH = 11.21 (iii) (iv) (v) phosphate buffer pH = 6.96 human urine pOH = 7.8 tomato juice pOH = 9.9The following two reactions involve proton transfer. In each reaction, identify the acid and the base. Identify the conjugate base of the acid, and the conjugate acid of the base. Draw Lewis electron dot diagrams for each molecule, and describe the rear- rangement of bonding in the reaction as nonbonding electron pairs become cova- lently shared pairs and vice versa. (a) H¿O(€) + NH (aq) → H;0* (aq) + NH3(aq) (b) CH;CH;OH(aq) + NH7 (aq) → CH;CH;O¯(aq) + NH3(aq)Write and balance equations for the following acid-base neutralization reactions: