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chemistry
Consider 18.0 M H2SO4, if you need to make 250.0 mL of a 3.0 M solution of H2SO4, how would you do this? 18.0 M H2SO4 has a density of 1.84g/mL what is the molality of solution? Mass % of H2SO4 in the solution and the mol fraction
asked by Marie on April 29, 2013 
Chemistry
Consider 18.0 M H2SO4, if you need to make 250.0 mL of a 3.0 M solution of H2SO4, how would you do this? 18.0 M H2SO4 has a density of 1.84g/mL what is the molality of solution? Mass % of H2SO4 in the solution and the mol fraction
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A 25mL sample of 0.160M solution of NaOH is titrated with 17 mL of an unknown solution of H2SO4. What is the molarity of the sulfuric acid solution? A. 0.004M H2SO4 B. 0.235M H2SO4 C. 0.117M H2SO4 D. 0.002M H2SO4
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Suppose you wanted to produce 1.17 L of a 3.41 M aqueous solution of H2SO4. How many grams of solute are needed to make this solution? (H2SO4)
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5.0 mL of H2SO4 solution was titrated with 0.20 M NaOH standard solution. The volume of NaOH needed to reach the equivalent point was 9.5 mL. 1. In this titration setup, what is the titrant? and what is the analyte? 2. What is the
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how much volume of h2so4 is needed to produce a 0.953 Normality) of h2so4 if the 1 liter solution is 1.14 g/mL in density?
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An aqueous solution that is 30.0 percent sulfuric acid (H2SO4) by mass has a density of 1.105 g/mL. Determine the molarity of the solution.
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An aqueous sulfuric acid solution containing 571.6 g of H2SO4 per liter of solution at 20°C has a density of 1.3294 g/mL. Calculate (a) the molarity, (b) the molality, (c) the percent by mass, and (d) the mole fraction of H2SO4
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A 21.18 mL of 0.250 M NaOH is titrated with a H2SO4 solution. The initial volume of H2SO4 was 13.28 and the final volume of H2SO4 was 28.29 mL when the solution turned very slightly pink. What is the concentration of H2SO4?
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