Don't used hand raiting -1A certain liquid X has a normal freezing point of 1.60 °C and a freezing point depression constant K, = 1.52 °C·kg·mol . A solution isprepared by dissolving some barium hydroxide (Ba(OH)2) in 700. g of X. This solution freezes at 0.6 °C. Calculate the mass ofBa(OH)2 that was dissolved.Round your answer to 2 significant digits.☐ g☐ x10xG

The freezing point depression formula: ΔTf = i Kf mWhere:ΔTf is The freezing point depression.i is…

Answered: -1 A certain liquid X has a normal…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter4: Energy And Chemical Reactions

Section: Chapter Questions

Problem 120QRT

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A soft drink contains an unknown mass of citric acid, C3H5O(COOH)3. It requires 6.42 mL of 9.580 × 10−2-M NaOH to neutralize the citric acid in 10.0 mL of the soft drink. C3H5O(COOH)3(aq) + 3 NaOH(aq) → Na3C3H5O(COO)3(aq) + 3 H2O(ℓ) Determine which step in these calculations for the mass of citric acid in 1 mL soft drink is incorrect? Why? n (NaOH) = (6.42 mL)(1L/1000 mL)(9.580 × 10−2 mol/L) n (citric acid) = (6.15 × 10−4 mol NaOH) × (3 mol citric acid/1 mol NaOH) m (citric acid in sample) = (1.85 × 10−3 mol citric acid) × (192.12 g/mol citric acid) m (citric acid in 1 mL soft drink) = (0.354 g citric acid)/(10 mL soft drink) Determine the correct result.
What mass of solid NaOH (97.0% NaOH by mass) is required to prepare 1.00 L of a 10.0% solution of NaOH by mass? The density of the 10.0% solution is 1.109 g/mL.
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Suppose 1.24 g of sodium chloride is dissolved in 200. mL of a 28.0 m M aqueous solution of silver nitrate. Calculate the final molarity of sodium cation in the solution. You can assume the volume of the solution doesn't change when the sodium chloride is dissolved in it. Be sure your answer has the correct number of significant digits. ol M x10 Ar
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