what’s the ph of 0.2M solution of H2SO4? presumed that the sulfuric acid will easily give...
1) 10ml of 0.1M Nitric Acid is added to 20ml of 0.2M Sulfuric (H2SO4) and then diluted up to 100 ml, what is the resulting pH? Hint: Recall [H3O+] = total moles of [H+]/total Volume 2) Which of the following acid solutions is the MOST acidic? (careful it’s a mix of concentrations as well as Ka and pKa) a) 1.0M Phenol, Ka = 1.3 x 10-10 b) 0.08M Pyruvic acid, pKa = 2.76 c) 0.1M Bromo-Acetic acid pKa =...
A) Considering the dissociation reaction for sulfuric acid in water, what is the pH of a 1.00 x 10^-2 M solution of H2SO4? B) HSO4- will hydolize in water to produce additional H30+; its Ka = 1.2 x 10^-2. Recalculate the pH of the 1.00 x 10^-2 H2SO4 solution, this time also considering the additional H30+ produced from the reaction.
a sulfuric acid solution containing 551.5
(a) A sulfuric acid solution containing 551.5g of H2SO4 per liter of Solution has a density of 1-339 Icme. Calculate molality of HaSO4 in this solution. the
What is the PH of a 100 mM solution of sulfuric acid (H2SO4)? Ka1=Large Ka2=1.2x10^-2 A. 2.02 B. -0.96 C. 1.00 D. 1.9 E. 0.96
A. Calculate the pH of a solution containing 0.2M lactic acid (pKa = 3.86) B. Calculate the pH of a solution of 1x10^-9 M HCl (strong acid) in distilled water. Show your work.
instructions 1 pts Question 4 Concentrated sulfuric acid is 18.1 M. The first hydrogen is a strong acid and is completely ionized, the second hydrogen is a weak acid with a K 2 = 0.012 If only the first hydrogen ionized the pH would be pH = -log(18.1) = -1.258. When we include the partial ionization of the second hydrogen, what is the pH of this solution? • Previous MacBook |
A solution is prepared by dissolving 27.75 g sulfuric acid, H2SO4, in enough water to make exactly 200.0 mL of solution. If the density of the solution is 1.1094 g/mL, what is 1. Weight % of H2SO4 in the solution? 2. Mole fraction of H2SO4 in the solution? 3. Molarity of H2SO4 in the solution? 4. Molality of H2SO4 in the solution?
A solution is prepared by dissolving 27.75g Sulfuric Acid, H2So4 in enough water to make exactly 200. mL of solution. If Density = 1.1094g/mL What is the Mole Fraction of H2S04?
A.) An aqueous solution of sulfuric acid is made by dissolving 585.0 g of sulfuric acid in enough distilled water to make a one liter solution. Calculate the molarity, the molality, the mass% and the mole fraction of sulfuric acid in this solution. The density of this solution is 1.350 g/mL. MW H2SO4 = 98.00 g/mol. Please explain!! Thank you B.) Which substance(s) is (are) miscible in water? CH3CH2OH CI4 C6H6 CH3(CH2)13CH2OH CH3OH HOCH2CH2OH
A solution is prepared by dissolving 17.75 g sulfuric acid, H2SO4, in enough water make 100.0 mL. What is the molarity? A) 1.940 M H2SO$ B) 0.1810 M H2SO4 C) 1.810 M H2SO4 D) 0.1775 M H2SO4