Consider the following data on some weak acids and weak bases: acid name acetic acid hypochlorous acid solution 0.1 M KCIO 0.1 M CH NHyCl Use this data to rank the following solutions in order of increasing pH. In other words, select a 'I' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. 0,1 M Nar K₂ formula HCH₂CO₂ 1.8 x 105 HCIO 3.0 x 108 0.1 M NaCH₂CO₂ X PH 1 (lowest) choose one choose one choose one base K₂ formula pyridine CHN 1.7 * 10⁹ aniline CH₂NH₂ 4.3 × 10 ¹0 name

Determine the pH of each solution.       Part A 0.13 M NH4Cl (Kb(NH3)=1.76×10^−5)   0.18 M NaC2H3O2 (Ka(HC2H3O2)=1.8×10^−5) 0.19 M NaCl

Calculate the pH AND the pOH of each of the following solutions 9) 150,000 mL of a solution containing 45 grams of HNO3 (nitric acid) and 998 grams of hydrobromic acid. 10) 5.0 L of a solution containing 0.09 grams of sodium hydroxide, 0.9 grams of lithium hydroxide, 9.0 grams of barium hydroxide, and 90.0 grams of potassium hydroxide (KOH). Solve the following acid-base reaction and THEN determine the pH and pOH of the solution after the reaction has come to completion. 11) A 110.0 mL aqueous solution of 0.51 M Ba(OH)2 is added to a 220.0 mL aqueous solution of 0.15 M H3PO4. (What kind of stoichiometry problem is this?)

Arrange the following solutions in increasing order of their pH. 0.1 M NaCl 0.1M C,H;NH,Br 0.1M C,H,NH,CI 0.1M NaF Use the following data to answer the question: K, of HF is 6.8×10*, K, of aniline is 4.3 x10-1º, K, of ethylamine is 6.41x10-4 (A) 0.1M C,H, NH,Cl < 0.1M C,H,NH,Br < 0.1 M NaCl < 0.1M NaF (B) 0.1M C,H,NH,Cl < 0.1M C,H,NH,Br < 0.1M NaF < 0.1 M NaCl (C) 0.1M C,H,NH,Br < 0.1M C,H,NH,Cl < 0.1 M NaCl< 0.1M NaF (D) 0.1M C,H;NH,Br < 0.1M C,H;NH,Cl < 0.1M NaF < 0.1 M NaCl