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Chemistry: Ammonium Meta Tungstate

AMT (ammonium meta tungstate) has a MW of 2956.2 g/mol. Calculate the amount of AMT (in grams) needed to be dissolved in water that would give a 0.2 M AMT aqueous solution.

Also on an unrelated problem, how would you dilute (with water) 12.1 Normality HCl and 14.8 Normality NH4H2O to give 1M HCL and 1M NH4H20 respectively?

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Question 1:

AMT (ammonium meta tungstate) has a MW of 2956.2 g/mol. Calculate the amount of AMT (in grams) needed to be dissolved in water that would give a 0.2 M AMT aqueous solution.

Answer:

The molar concentration of a solution (M) represents the number of moles dissolved in one liter of solution (usually water). So an 0.2M solution of AMT would contain 0.2 moles in 1 liter of water.

The molecular weight of a compound or element is calculated from it's chemical formula (sum of the atomic weights of the constituent atoms). The molecular weight of ammonium meta tungstate (NH4)6H2W12O40 is calculated by summing the individual atomic weights (2956.2 amu).

The molecular weight of a single atom is small* ...

Solution Summary

This solution provides a detailed explanation of the two given chemistry problems.

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