If 880 mL of water is added to 125.0 mL of a 0.770 M HBrO 4 solution what is the resulting molarity?

If 880 milliliters of water is added to a 125 milliliters of a 0.770 molar perbromic acid solution, what is the resulting molarity? Alright. So they're saying we're adding water to it, so that's clearly a dilution. So m 1v1 equals m 2v2. They're asking us what's the resulting solution after I've added water. So So they're asking what is the diluted concentration. So we're looking for m 2. That would mean that this first molarity given to us would have to be m 1. It's multiplying with v 1. Now, 880 ml of water added is not v 2. Remember, v 2 represents your final volume. V 2 equals your initial volume plus the volume of water that has been added. So v 2 is actually 1 25 milliliters plus the 880 ml's of water added. So v 2 is actually 1,005 milliliters. So that's what we're gonna plug here. We're going to divide both sides now by 1,005 milliliters. When we do that, we see that our milliliters cancel out and we'll have m 2 at the end. When you plug this in, you'll get 0.0958 molar for your new molarity. Now technically here this is 880 milliliters, so that's 2 significant figures. So So we could round this to 0.096 molar. So that would be the resulting molarity after I've added 880 milliliters water to my original solution.

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9. Solutions

Dilutions

GOB Chemistry

9. Solutions

Dilutions

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Multiple Choice

If 880 mL of water is added to 125.0 mL of a 0.770 M HBrO₄ solution what is the resulting molarity?

0.096 M

0.136 M

0.257 M

0.892 M

1.76 M

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Verified step by step guidance

Start by understanding the concept of dilution, which involves adding solvent to a solution, decreasing the concentration of the solute.

Use the dilution formula: \( M_1V_1 = M_2V_2 \), where \( M_1 \) and \( V_1 \) are the initial molarity and volume, and \( M_2 \) and \( V_2 \) are the final molarity and volume.

Identify the initial conditions: \( M_1 = 0.770 \) M and \( V_1 = 125.0 \) mL. Calculate the total final volume \( V_2 \) by adding the initial volume to the volume of water added: \( V_2 = 125.0 \) mL + \( 880 \) mL.

Substitute the known values into the dilution formula: \( 0.770 \times 125.0 = M_2 \times (125.0 + 880) \).

Solve for \( M_2 \) to find the resulting molarity after dilution.