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  • A mass of 3214 g of sodium bicarbonate was dissolved and diluted to 250.00 ml of aqueous solution. A 29.55OX mL of sodium bicarbonate solution was used to neutralise

25.00 ml of H2SO4 solution during a titration. Calculate the molar concentration of H2SO4 solution.

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Related questions

Concentrated sulfuric acid (18.4-molar H2SO4) has a density of 1.84 grams per milliliter. After dilution with water to 5.20-molar, the solution has a density of 1.38 grams per milliliter and can be used as an electrolyte in lead storage batteries for automobiles. (a) Calculate the volume of concentrated acid required to prepare 1.00 liter of 5.20-molar H2SO4. (b) Determine the mass percent of H2SO4 in the original concentrated solution. (c) Calculate the volume of 5.20-molar H2SO4 that can be completely neutralized with 10.5 grams of sodium bicarbonate, NaHCO3. (d) What is the molality of the 5.20-molar H2SO4?

A weighed amount of sodium chloride is completely dissolved in a measured volume of 4.00 M ammonia solution at ice temperature, and carbon dioxide is bubbled in. Assume that sodium bicarbonate is formed until the limiting reagent is entirely used up. The solubility of sodium bicarbonate in water at ice temperature is 0.75 mol per liter. Also assume that all the sodium bicarbonate precipitated is collected and converted quantitatively to sodium carbonate. The mass of sodium chloride in (g) is 14.3 The volume of ammonia solution in (mL) is 29.8 Calculate the following How many moles of ammonia are present originally? what is the limiting reagent? a) ammonia b) sodium chlorideWhat is the theoretical yeild of sodium bicarbonate in grams? How many grams of the sodium bicarbonate formed will precipitate from the above volume of solution? How many grams of sodium carbonate will be produced from this precipitate??
A weighed amount of sodium chloride is completely dissolved in a measured volume of 4.00 M ammoniasolution at ice temperature, and carbon dioxide is bubbled in. Assume that sodium bicarbonate is formeduntil the limiting reagent is entirely used up. The solubility of sodium bicarbonate in water at ice temperatureis 0.75 mol per liter.Also assume that all the sodium bicarbonate precipitated is collected and converted quantitativelyto sodium carbonateThe mass of sodium chloride in (g) is 14.3The volume of ammonia solution in (mL) is 29.8Calculate the followingHow many grams of the sodium bicarbonate formed will precipitate from the above volume of solution?How many grams of sodium carbonate will be produced from this precipitate??

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