# Chem- PLZ HELP!

Consider 100g of 5.5% (mass) solution of NaNO3. Complete the following table, before calculating molarity, molality and mole fraction of NaNO3.

Solute(NaNO3)|Solvent(H2O|Soln
Mass(g) 100g

Moles ----

RefInfo 85g/mol 18.02g/mol

Density=1.00g/mol (This goes under "soln" as reference info).

Ok well I attempted to make a table. I have to fill it in. Can anyone help me fill it out plz?

1. 👍 0
2. 👎 0
3. 👁 238
1. Ok that looks wrong.

100g should be under solution for the mass, 18.02g/mol for the solvent of H2O and 85g/mol for the solute of NaNO3. I have to find mass of solute and solvent and the moles of solute and solvent. Pls help anyone!

1. 👍 0
2. 👎 0
2. I can't make out some of it but I can get you started and you can fill in the missing parts.
100 g NaNO3 solution that is 5.5% w/w.
That is NOT 100 g NaNO3, that is 100 g of the solution.
5.5% w/w means 5.5 g NaNO3/100 g solution.

So mass solute = 5.5 grams.
moles solute = 5.5/molar mass NaNO3.
mass solution = 100 g
mass solute = 5.5
mass solvent (H2O) = 100-5.5 = ??
moles solvent(H2O) = g solvent/molar mass solvent.

1. 👍 0
2. 👎 0

## Similar Questions

1. ### Chemistry

An 8.00 mass % aqueous solution of ammonia has a density of 0.9651g/ml. Calculate the molality, molarity, and mole fraction of NH3. This question seems simple but I cannot seem to remember how to do this. Help please?

2. ### Chemistry

The density of an aqueous solution containing 10% of ethanol (C2H5OH) by mass is 0.984 g/ml. A) Calculate the molality of this solution. B) Calculate its molarity. C) What volume of the solution would contain 0.125 mol of ethanol.

3. ### Chemistry

An aqueous KNO3 solution is made using 72.5 grams of KNO3 diluted to a total solution volume of 2.00 liters. If the molarity of the solution is .359 M and the molality of the solution is .354, what is the mass percent of the

4. ### AP Chemistry

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

1. ### Chemistry

Calculate the molarity and the molality of an NH3 solution made up of 30 g of NH3 in 70 g of water. The density of the solution is 0.982 g/ml. Molar Mass of NH3 = 17.04 g

2. ### chemistry

1.)An aqueous solution is 34.0% H3PO4 by mass and has a density of 1.207 g/mL. What is the molarity of the solution? AND what is the molality?

3. ### chemistry

Finding molarity and molality(best answer)? An aqueous solution is prepared by diluting 3.30 mL acetone,(d= 0.789g/mL) with water to a final volume of 75.0 mL. The density of the solution is 0.993 g/mL. What is the molarity,

4. ### college chem

. Jack Daniels Tennessee whiskey is 40.00% ethanol by volume. However, % alcohol by mass is quite different from % by volume. The molality of ethanol in an aqueous solution that is 40.00 % ethanol by volume is 10.88 molal. A) Find

1. ### chemistry

the density of an aqueous solution containing 10.0% by mass ethanol is 0.984 g/ml. calculate molality and molarity. what volume of the solution would contain 1.15 g ethanol ?

2. ### Chemistry

An aqueous solution is 8.50% ammonium chloride, NH4Cl, by mass. The density of the solution is 1.024g/mL. Calculate the molality, mole fraction, and molarity of NH4Cl in the solution. I know the formulas needed but I'm not sure

3. ### chemistry is this answer right

115 grams of KCl is dissolved in 750 ml of water. what are the molality, molarity, mole percent, % mass, ppm by mass. what would the freezing point and boiling point of that solution assuming Kf of water is 1.86 degree celsius/m

4. ### chemistry

Find the molar masses of the following compounds: 1. LiI 2. PbCO4 3. Mg(OH)2 4. (NH4)3PO4 Find the percent composition (percent by mass) of the given element in the following compounds: 1. Fluorine in AgF 2. Hydrogen in glucose