Chemistry - pH practice Calculate the following: 1. What is the pH of a solution where: a) [H+] = 4.3x10 [H+] = 7.6x10-10 b) [OH-]= 8.4x10 00 [OH-]= 2.2x10 c) POH = 8.3 1) POH = 3.7 2. What is the [H+] of a solution where: a) pH=11.2 d) pH = 3.6 b) pOH = 9.4 e) pOH = 2.2 c) [OH-]=6.2x10" f) [OH-]=1.8x10 3. What is the pH of a 0.05M HCI solution? 4. What is the pH of a 0.05M NaOH solution? Acid-Base Equilibrium - SET I pH = -log[H+] POH = -log[OH-] 10 [H+][OH-] [OH-]=1000 [H+] = 10H KKK 1. Complete the following using the given piece of information: a) [H+] = [OH-] = pH= POH = 4 b) [H+] = 1 x10 [OH-]= pH= POH = c) [H+] = [OH-] = pH = 9 POH = d) [H+] = [OH-]= pH = POH = 5 e) [H+] = [OH-]= 10 pH= POH = f) [H+] = [OH-] = pH = 2 POH = 2. Differentiate between a strong and weak acid. 3. Complete the following acid/base ionization reactions. In each case, a conjugate acid and bose are produced. a) H25() HO b) CHNH HO c) HCO3) H₂O) d) CO H₂O e) NH3(00) H₂O 4. For each the following solutions calculate: α) 0.0001 Μ ΗΙ [H+] = [OH-] = pH = POH = b) 0.1 M KOH [H+] = [OH-]= pH = POH= c) 0.001 MHNO, [H+]= [OH-] = pH= POH = d) 0.002 M Mg(OH) [ H+] = [OH-]= pH= POH= 5. What is the conjugate acid of: a) OH b) NH c) HPO d) H₂O 6. What is the conjugate base of: a) H₃PO₄ b) NH c) HPO d) OH Chemistry pH, Strong Acid Strong Base Neutralization Reactions 1. Complete the following: a) [H+] = [OH-] = pH= POH = 4.4 b) [H+] = 1.8x10 [OH-] = pH= POH = c) [H+] = [OH-]= pH = 9.2 POH = d) [H+] = [OH-] = pH= POH = 5.7 e) [H+] = [OH-] = 8.4x10 pH= POH = 1) [H+] = [OH-]= pH = 2.6 POH = 2. Predict the results of the following hydroxide neutralization reactions; then balance the equations. HCI + NaOH → H₂SO₄ + HI + Mg(OH)2→ HCIO + NHOH→ 3. Complete and balance the following equations, then answer the question that follows. HBrO + LIOH→ If it takes 25.5mL of 0.2M LIOH to completely neutralize 15.0ml. of a sample of the strong acid HBrO4, what is [HBrO]? pH? H₂SO₄ + NaOH -> What is the molarity of a NaOH solution if it takes 8.7mL of a 0.1M H₂SO₄ solution to neutralize a 15ml sample of the NaOH? pH? HNO3 + Ba(OH)2→ A 10mL sample of Ba(OH), is titrated to its endpoint with 16.4mL of 0.05M HNO3. What was the concentration of the Ba(OH)2 solution? pH? Brönsted/Lowry Theory Practice Acid Base Questions 1. In a weak acid (HA) solution, how do the number of HA molecules compare to the number of H lons present? 2. Write a balanced equation for the ionization of: (a) HCN + H₂O (b) NH₂ (base) + H₂O (c) HBr + H₂O (d) CH3NH2 (base) + H₂O 3. Arrange the following 1.0 M solutions in order of decreasing pH. (Hint: what are their K's?) CHCOOH, H₃PO₄, LIOH, NH, Highest pH Lowest pH 4. What kind of relationship is there between the [H+] and [OH-]? Explain... 5. Complete the following ionization reactions: (a) Hlaq) + H2O (b) CH3NH2+H₂O (base) (c) HNO2(aq) + H2O (d) NH₃+ H₂Om (base) 6. Give an example of: (a) a strong acid (b) a strong base (c) a weak base 7. Give the conjugate base for: (a) H₃PO (b) HCO 8. Give the conjugate acid for: (a) OH (b) SO