A 0.705 g sample of unknown metal phosphate compound was reacted with excess silver nitrate resulting in 0.674 g of silver phosphate precipitate. Calculate the percent by mass of the phosphate in the original unknown metal phosphate compound.
A 0.705 g sample of unknown metal phosphate compound was reacted with excess silver nitrate resulting in 0.674 g of silver phosphate precipitate. Calculate the percent by mass of the phosphate in the original unknown metal phosphate compound.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Question
so I have a couple questiond actually
1. A 0.705 g sample of unknown metal phosphate compound was reacted with excess silver nitrate resulting in 0.674 g of silver phosphate precipitate. Calculate the percent by mass of the phosphate in the original unknown metal phosphate compound.
2. Calculate the grams of potassium sulfate required to make 250.0 mL of a 0.0300 M solution.
3. Determine the molecular formula for a compound consisting of 95.21% carbon and 4.79% hydrogen with a molecular mass of 252.30 g/mole.
4. What total volume must 85.0 mL of 1.30 M phosphoric acid solution be diluted to prepare 0.650 M phosphoric acid solution?
5. 0.330% of the mass of a hemoglobin molecule is iron. Calculate the number of iron (II) ions per molecule of hemoglobin. Hemoglobin has a molecular mass of 6.80 x104 g/mole.
Expert Solution
Step 1
Mass of metal phosphate = 0.705 g
Mass of silver phosphate = 0.674 g
We need to find the percentage of phosphate in original compound.
Note : Since there are multiple questions as per guidelines I can answer only first one. Please post others seperately. Thank you.
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