Answer the following questions about weak acids. Use the K values in the following table to help answer some of the questions. Acld Ko HF 6.7 x 10-4 HC2H3 O2 1.8 x 10-5 (b) Which solution has a higher percent ionization of the acid, a 0.10M solution of HC2H3O2 (aq) or a 0.010 M solution of HC2H3 02 (ag) ? Justify your answer including the calculation of percent ionization for each solution. 1 Upload files (PDF, JPG, GIF, PNG, TXT, Word, Excel, Powerpoint, file formats supported)

Write separate equations representing the reaction of H2 PO4−(a) as a base with HBr(b) as an acid with OH−

H2C2O4 is a diprotic acid that dissociates as shown below.Ka1 = 5.38 x 10-2 and Ka2 = 5.18 x 10-5. Determine the pH of 0.1 M Sodium hydrogen oxalate (NaHC2O4). (Note: neglect hydroxide formation due to hydrogen oxalate  hydrolysis)

7 (a) Describe what happens when each of the following molecules is separately dissolved in water and illustrate with an equation in each case: (i) ethavois acid (CH;COOH) (ii) ammonia (NH3) (b) Identify the conjugate acids and bases in the substances mentioned in question 7(a) above.

For the following reaction, which species functions as the acid? Xoo Хон (C) (A) + (B) + (D)

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The pH of a 1.00 M NaCH3COO (aq) solution is 9.38. a/ Determine the concentration of [OH-] in the solution.  b/ Write the expression for the Kb of NaCH3COO (aq) and calculate its values.  c/ Calculate the pKa of CH3COOH. d/ HCl (aq) is added to 1.00 L solution of 1.00 M NaCH3COO (aq). Write the chemical reaction between HCl (aq) and NaCH3COO (aq).  e/ How many mol of HCl (aq) is needed to make a buffer solution with pH = 5.00 from 1.00 L of 1.00 M NaCH3COO (aq).

Rank the following aqueous solutions in terms of pH. Why Are they in that order? (a)0.1 M CH3COOH (b)0.1 M H2SO4 (c)0.1 M HNO3 (d)0.1 M CH3COOH + 0.1 M CH3COONa (e)0.1 M HF (f)0.1 M HCl

Calculate the molar concentrations of oxalic acid (COOH)2, HOOCCO2-, (CO2)22-, H3O+, and OH- in 0.15 M (COOH)2 (aq). This is a special case of general diprotic acid dissociation. First, we need to find the pKa1 and pKa2 in the water at room temperature, which is available in the textbook page 192 table 8.2. It is also available online e.g. Wikipedia (oxalic acid). pKa1 = 1.23, pKa2 = 4.19. Either solve numerically or analytically. Report here [H3O+] = ______ M.  2 sig. figures.

If the pH of a 0.0850 M solution of HBRO2 is 2.29, then what is the value for the acidity constant, Ką, of HBRO2? HBrO2(aq) + H2O(1) H3O*(aq) + BrO2 (aq) K¸ = ? K, for HB1O2: