calculate the mass in grams of BaSo4 that was formed from the following information.
Moles of Ba(OH)2 = Moles BaSo4
volume Ba(OH)2 dispensed = 10 ml
Molarity of H2SO4 used = 0.100 M
Molarity of Ba(OH)2 solution = 0.118 M
calculate the mass in grams of BaSo4 that was formed from the following information. Moles of Ba(OH)2 = Moles BaSo4 volu...
Q6. A student mixes 50.0 mL of 1.00 M Ba(OH)2 with 86.4 mL of 0.494 M H2SO4. Calculate the mass of solid BaSO4 formed and the pH of the mixed solution
Be sure to answer all parts. A student mixes 50.0 mL of 1.00 M Ba(OH)2 with 76.2 mL of 0.450 M H2SO4. Calculate the mass of BaSO4 formed. g Calculate the pH of the mixed solution.=
50.0 mL of 1.00 M Ba(OH)2 is mixed with 81.6 mL of 0.450 M H2SO4. Calculate the pH of the solution after BaSO4 precipitates. 1.00 13.31 13.00 0.69 13.88
A. How many milliliters of 0.110 M HCl are needed to completely neutralize 55.0 mL of 0.107 M Ba(OH)2 solution? Express the volume in milliliters to three significant digits. B. How many milliliters of 0.125 M H2SO4 are needed to neutralize 0.170 g of NaOH? Express the volume in milliliters to three significant digits. C. If 55.0 mL of BaCl2 solution is needed to precipitate all the sulfate ion in a 746 mg sample of Na2SO4, what is the molarity of the solution? Express the molarity...
2(10 points) A solution is prepared by dissolving 25.00 grams o f ba rium nitrate, Ba(NO) in sufficient water to make 500.0 mL of solution. A 25.0 mL sample of this is diluted with water to a final volume of 200.0 mL. What is the molarity of the final solution? (Ba(NO>-398.6 g/mol) 3. (10 points) Consider a solution prepared by mixing 349 grams of methanol, CHOH CHOH-320 g/mol) and 750 grams water. The final volume of the solution is 1105...
Consider the following reaction: Ba(OH)2 (aq) + H2SO4 (aq) ⟶ BaSO4 (s) + 2 H2O (l) If you add an excess of sulfuric acid to 85.67 g of barium hydroxide, how many grams of water will you expect to produce?
How many grams Ba(NO3)2 of are required to precipitate all the sulfate ion present in 15.3 mL of 0.143 M H2SO4 solution? Ba(NO3)2 + H2SO4 --> BaSO4 + 2HNO3
This experiment involves the reaction of Ba(OH)2 with H2SO4. Which of the following gives the balanced chemical reaction used in the experiment? BaSO4(s) + 2 H2O(l) → Ba(OH)2 (aq) + H2SO4(aq) Ba(OH)2 (aq) + H2SO4(aq) → BaSO4(s) + 2 H2O(l) Ba(OH)2 (aq) + H2SO4(aq) → BaSO4(s) + H2O(l) Ba(OH)2 (aq) + H2SO4(aq) → H2Ba(s) + SO4(OH)2(l) Which of the following gives the net ionic reaction for the reaction used in this experiment? Ba2+(aq) + 2 OH-(aq) + 2 H+(aq) +...
2. A precipitate is formed when 2.27 L of 0.0820 M Ba(OH)2 are mixed with 3.06 L of 0.0664 M N^2SO4 based upon the equation below Ba(OH)2(aq)Na2SO4(aq) > BaSO4(s) + 2 N2OH(aq) What is the mass of the precipitate formed from the Ba(OH)2? (Show all work) What is the mass of the prccipitatc formcd from thc Na2SO4? (Show all work) What is the limiting reactant? What is the theoretical yield of the precipitate?
4. What volume (in L) of 0.586 M Ba(OH)2 (aq) contams V.* of Ba(OH)2 dissolved in it? 5. If 16.0 mL of water are added to 31.5 mL of 0.586 M Ba(OH)2 (aq), what is the new solution molarity?