2)
1) balanced equation :
2 HC2H3OS (aq) + Ba(OH)2 (aq) ------------> Ba(C2H3OS)2 (aq) + 2 H2O (l)
2)
pH = 1/2 (pKa - log C)
= 1/2 (3.33 - log 0.6)
pH = 1.78
B. 15 points) What is the hydronium ion concentration of a 0.20 M Solution of trimethylamine (CH3)N; Ko = 7.4 x 103...
ASAP Part short w points Show your work dearly and provided Heart answers with its where pe 12A solutions paredad ml of 3x10M NOH will cdo what is the lon product for Carou T 2.5x19 LOYMEN precipitatier this will it precipitate? Circle ong: Yes No f on product: 8.15 points) What is the hydronium ion concentration of a 0.20 M solution of trimethylamine (CH), NK - 7.4 x 10 Hydronium ion concentration O ) C (5 points) What is the...
The hydronium ion concentration of an aqueous solution of 0.333 M trimethylamine (a weak base with the formula (CH3)3N) is [H3O+] = M
The hydroxide ion concentration in an aqueous solution at 25°C is 4.4x10-2 M. The hydronium ion concentration is M. The pH of this solution is The pOH is The hydronium ion concentration in an aqueous solution at 25°C is 4.4x10 M. The hydroxide ion concentration is M. The pH of this solution is The pOH is Autoionization occurs when two solvent molecules collide and a proton is transferred between them. Write the autoionization reaction for water. Submit Answer Use pH,...
The hydronium ion concentration of an aqueous solution of 0.461 M diethylamine (a weak base with the formula (C2H5)2NH) is [H3O+] = _____M. The hydroxide ion concentration, [OH-], of an aqueous solution of 0.461 M trimethylamine (a weak base with the formula (CH3)3N) is ____M.
1. Calculate the hydronium ion concentration and the hydroxide ion concentration in lime juice with a pH of 2.0. Report answers in scientific notation and 2 significant figures Hydronium ion concentration = Hydroxide ion concentration = 2. What are the hydronium and hydroxide ion concentrations in a solution whose pH is 6.52? Report answers in scientific notation and 2 significant figures Hydronium ion concentration = Hydroxide ion concentration = 3. Which is the stronger acid, NH4+ or HBrO? Hint: Compare...
Find the hydronium ion concentration and pH for the following 1. 2. Calculate the hydronium ion concentration and the pH when 80.0 mL of 0.55 MNH, is mixed with 80.0 mL of 0.55 M HCl (K. = 5.6 x 10-10). Concentration M pH- Phenol (CH-OH), commonly called carbolic acid, is a weak organic acid. C, H, OH(aq) + H2O(0) = CH.0 (aq) +H3O+ (aq) K= 1.3 x 10-10 If you dissolve 0.593 g of the acid in enough water to...
3. Solution A has a hydronium ion concentration of 3.8 x 10® M. Solution B has a hydronium ion concentration of 2.5 x 10M. a. Which solution has the higher hydronium ion concentration? b. Which solution has the higher pH? C. Calculate the pH of the more acidic solution. Show all work. 4. Consider hydrolysis reactions and then predict whether the pH of an aqueous solution of each of the following compounds is greater than 7(>7), less than 7<7), or...
1) The hydroxide ion concentration in an aqueous solution at 25°C is 6.4×10-2 M. The hydronium ion concentration is M. The pH of this solution is ____. The pOH is _____. 2) The hydronium ion concentration in an aqueous solution at 25°C is 3.6×10-2M. The hydroxide ion concentration is _____M. The pH of this solution is ____ The pOH is ____ 3) What is the pOH of an aqueous solution of 0.467 M hydrochloric acid? pOH = ____ 4) What is...
The hydronium ion concentration in an aqueous solution at 25°C is 3.3x10 - M. The hydroxide ion concentration is M. The pH of this solution is The pOH is The pH of an aqueous solution at 25°C was found to be 6.00. The pOH of this solution is The hydronium ion concentration is The hydroxide ion concentration is The hydroxide ion concentration in an aqueous solution at 25°C is 6.3x10-2 M. The hydronium ion concentration is M. The pH of...
At 25 °C, a solution has a hydronium ion concentration of 2.70×10-8 M. What is the pH, pOH, and [OH-] of this solution? pH = ___________ pOH = _________ [OH-] = ________ M