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UN CUNCILIULUNU 64. Calculate the pH and the pOH of each of the following solutions at...
Be sure to answer all parts. Calculate the pOH and pH of the following aqueous solutions at 25 ° C: (a) 0.0775 M LiOH pH = pOH = (b) 0.0441 M Ba(OH)2 pH = pOH = (c) 0.25 M NaOH pH = pOH
Please help! will rate!! Calculate the [H.O*), (OH), pH, and pOH of each of the following solutions at 25°C. a. 0.25 M HCI b. 0.016 M Ba(OH), C. 0.30 M HCN d. 0.10 M H,SO
Activity #2 Calculate the pH of the following basic solutions. 1. Calculate the pH and pOH of a 0.200 M Ca(OH)2 2. Calculate the equilibrium concentrations for [OH-], [HB+), and [B], the pH and pOH for a 0.200 M pyridine solution. (CsH5N) Kb = 1.4 X 10-9 3. Calculate the equilibrium concentrations for [OH-], [HB], and [B], the pH and pOH for a 0.200 M methylamine. (CH3NH2) Kb = 4.4 X 10-4 4. Calculate the equilibrium concentrations for [OH-], [HB+],...
11. Calculate pH of the following solutions. At 25°C, Kw- [H30*] [OH'] = 1.00 x 10-14 pH=-log [H30 ] a) [H30 ] 2.30 x 10-12 M pOH=- log [OH] pH+ pOH = 14 b) [OH]=9.7x 102 M
Calculate the pOH and pH of the following aqueous solutions at 25 degrees Celcius (a) 0.0615 M LiOH (b) 0.0441 M Ba(OH)2 (c) 0.25 M NaOH
Calculate [OH − ], pOH, and pH for each of the following. (Assume that all solutions are at 25°C.) (a) 0.00023 M Mg(OH)2 [OH − ] pOH pH (b) a solution containing 17 g of KOH per litre [OH − ] pOH pH (c) a solution containing 170 g of NaOH per litre [OH − ] pOH pH
5. Calculate the pH for each of the following solutions a) pOH 4.72 b) 5.84 x 105 M HBr c) 8.62 x 10 M Sr(OH)2 d) [OH 3.77x 10-12 6. For each of the following reactions, identify the Lewis base, and also give the definition for a Lewis base. a) FeBr3 Br FeBr4 b) SO2+ H20- H2SO3 c) Hgl2 +2 I HgL d) H2OCN HCN+OH . For each of the following pairs of substances, identify the conjugate bases for each...
Listed below you will find concentration information about several aqueous acid-base solutions at 25°C. Match each acid base solution with the correct pH or POH - 0.78 M HCl(aq) 1.pOH = 8.28 . [H30+) = 1.7 * 10-5 M 2.pH = 13.48 .. [H30+1 -2.0 * 10-4 M 3.pH = 0.11 • 0.30 M NaOH(aq) 4. pOH = 10,30 [OH-] = 5.3 * 10-9M 5. pH = 4.77
Calculate the pH of each of the following strong acid solutions. (a) 0.00418 M HIO4 pH = (b) 0.365 g of HCIO4 in 25.0 L of solution pH = (c) 45.0 mL of 7.30 M HIO4 diluted to 4.50 L pH = (d) a mixture formed by adding 31.0 mL of 0.00172 M HIO4 to 28.0 mL of 0.00529 M HCIO4 pH =
Calculate the pH of each of the following strong acid solutions. Calculate the pH of each of the following strong acid solutions. (a) 0.00696 M HI pH = (b) 0.719 g of HCl in 29.0 L of solution pH = (c) 49.0 mL of 2.10 M HI diluted to 3.40 L pH = (d) a mixture formed by adding 87.0 mL of 0.000520 M HI to 47.0 mL of 0.000860 M HCI pH =