Calculate the milliliter of 2.00 M sulfuric acid needed completely neutralize 0.0500 L of 1.00 M of potassium hydroxide
Answer: 12.5 mL
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Calculate the milliliter of 2.00 M sulfuric acid needed completely neutralize 0.0500 L of 1.00 M...
A.How many milliliter of 0.125 M HCl are needed to completely neutralize 58.0 mL of 0.106M Ba(OH)2 solution? B. How many milliliter of 0.129 M H2SO4 are needed to neutralize 0.150g of NaOH? C. If 56.4mL of Bacl2 solution is needed to precipitate all the sulfate ion in a 748mg sample of na2 so4, what is the molarity of the solution? D. If 43.0ml of 0.208 M HCl solution is needed to neutralize a solution of Ca(OH)2 how many grams...
What volume of 0.2478 M sulfuric acid is required to neutralize 10.0 mL of 0.2662 M potassium hydroxide, KOH?
Part A. Calculate the volume lf 0.210-M NaOH solution needed to completely neutralize 89.1 mL of a 0.310-M solution of the diprotic acid H2C2O4 Part B. You wish to make a 0.202 M Hydrochloric acid solution from a stock solution of 3.00 M hydrochloric acid. How much concdntrated acid must you add to obtain a total volume of 50.0 mL of the dilute solution? Part C. an aqueous solution of barium hydroxide is standarized by titration with a 0.143 M...
38. Calculate the number of mL of 1.00 M sulfuric acid solution necessary to completely react with 40.0 mL of 0.250 M barium chloride solution? A) 8.25 mL B) 5.25 mL C) 10.0 mL D) 20.4 mL E) 40.8 mL
A) Balance the equation. B) 34.99 mL of 0.1001 M sodium hydroxide is needed to completely react (neutralize) 25.00 mL of sulfuric acid solution. What is the molarity of the sulfuric acid solution? _H2SO4(aq) _ NaOH(aq) Na2SO4(aq) + _H20(1) +
Calculate the volume of 0.510-M NaOH solution needed to completely neutralize 26.5 mL of a 0.860-M solution of the diprotic acid H2C2O4.
Calculate the volume of 0.660-M NaOH solution needed to completely neutralize 49.6 mL of a 0.460-M solution of the diprotic acid H2C2O4.
How many mL of 0.0946 M NaOH are needed to neutralize 25.0mL of 0.0750 M sulfuric acid?
5. Sodium bicarbonate (baking soda) will neutralize sulfuric acid according to the following reaction: 2 H200) + 2 CO2()+ Na2SOs(aq) 2 NAHCO3(aq)+H2SO4(aq) If a student spills 250.0 mL of sulfuric acid, how many grams of sodium bicarbonate should they use in order to completely neutralize it? Assume the density of sulfuric acid is 1.84 g/m L.
Calculate the theoretical number of mL of 0.200 M HCI needed to completely neutralize the weak base in the 25.0 mL of buffer. From your graph, determine how many mLo 0.200 MHCI were actually used to neutralize the base in the buffer. Compare this value to the calculated value. Did your buffer resist change in pH for the entire titration? Explain. Calculate how many moles of acid were added to reach the capacity of the buffer