chemistry

What would be the molarity of solution obtained by mixing equal volumes of 30% by mass H2SO4 (d=1.218 g/mL) and 70% by mass H2SO4 (d=1.610 g/mL). If the resulting solution has density 1.425 g/mL, calculate its molarity

1. 👍
2. 👎
3. 👁
1. Equal volumes will average the % HCl so (30+70)/2 = 50% HCl.
mols in 1000 mL will be
1.425 g/mL x 1000 mL x 0.50 x (1/36.5) = ?
And that's the M since mols/L = M.

1. 👍
2. 👎
2. The first question asks for the MOLARITY of the solution after adding the two together; the second question asks for the molarity using the DENSITY. You will get two different answers. Also, the acid that is given is H2SO4 and not HCl. The molecular weight that Drbob222 used to solve the problem will return the incorrect answer. Also, the addition of the two together will result in the acid being slightly higher than 50%, based on the density of the two acids.

1. 👍
2. 👎
3. Well, I screwed up big time. The problem says in big print H2SO4 and I used HCl.

1. 👍
2. 👎
4. part 2.
I looked up the %H2SO4 in density of 1.425 g/mL and it is 52.63%.
M H2SO4, then, is
1.425 g/mL x 1000 mL x 0.5263 x (1/98) = mols in 1 L and that is M.

1. 👍
2. 👎
5. I agree with DrBob222 and then I don't agree with him: I agree that the 2nd part that he gave you in his last point is correct, but the answer to part 2 isn't the answer to part 2. I agree that it should because adding these two concentrations of acid together doesn't produce a TOTAL VOLUME that is additive. For example, if you were to add 100mL of both acids together, the total volume should not be 200mL. But the way that the problem is worded, this is what I think that author of the question wants you to do for the first part. However, this is a poorly worded question and the second part is the correct way to determine the molarity of the acid, and not the way that it is implied in the first part.

1. 👍
2. 👎
6. I meant to say that the answer to part 2 isn't the answer to part 1.

1. 👍
2. 👎

Similar Questions

1. Chemistry

A solution is prepared by mixing 1.00g ethanol (C2H5OH) with 100.0g water to give a final volume of 101.mL. Calculate the molarity, mass percent and mole fraction of ethanol in the solution.

2. ap chemistry

a solution is prepared by mixing 50.0 mL toluene (C6H5CH3 d=0.867 g/mL) with 125 mL Benzene (C6H6 d=0.874 g/mL). assuming that the volumes add upon mixing, calculate the mass percent, mole fraction, molality, and molarity of the

3. chemistry

Assuming the volumes are additive, what is the [Cl-]solution obtained by mixing 210mL of 0.600M KCl and 630ml of 0.385M MgCl2 ?

4. Chemistry

An solution of antifreeze is prepared by mixing 23.0mL of ethylene glycol (d = 1.11 g/mL;molar mass = 62.07 g/mol) with 50.0 mL H2O (d = 1.00 g/mL) at 25°C. If the density of the antifreeze solution is 1.07 g/mL, what is its

1. chemistry

use the Henderson-Hasselbalch equation to calculate the pH of a buffer solution prepared by mixing equal volumes of 0.20 M NaHCO3 and 0.10M Na2CO3.(Ka=5.6x10^-11). how would you prepare NaHCO3-Na2CO3 buffer solution that has the

2. 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

3. Chemistry

If one assumes the volumes are additive, what is the concentration, in mol/L, of NO3− in a solution obtained by mixing 263 mL of 0.167 M KNO3, 311 mL of 0.404 M Mg(NO3)2, and 713 mL of H2O?

4. Chemistry

Use the concentrations and volumes of hydrogen peroxide and KI before mixing (Table 1), calculate the post-mixing concentrations. Before mixing: [H2O2] = 0.88M [KI] = 0.500M Table 1: before mixing 1. Vol H2O2 = 4.0 mL, [H2O2] =

1. chemistry

We are doing a lab that requires finding the molarity of an unknown AgNO3 solution after reacting NaCl + AgNO3 --> NaNO3 and AgCl and collecting/massing the precipitate. We will be using 10.00 mL of an NaCl solution and 10.00 mL

2. chemistry

What is the percent by volume (% v/v) of a solution made by mixing 12 ml of ethanol (C2H5OH) with 48 ml of water? b) Assuming the density of ethanol is 0.789g/ml, what is the molarity of this solution?

3. Chemistry

Suppose you are assigned to prepare a buffer of 0.10M HNO2 (Ka=1.7 x 10^-4) and 0.10M NaNO2 by mixing equal volumes of both solutions. What is the pH of the resultant solution? How would I first start this question? I have no clue

4. science

What is the Molarity of a solution formed by mixing 10.0g H2SO4 with enough water to make 100.0mL of solution?