If 920 mL of water is added to 78.0 mL of a 1.28 M HBrO 4 solution what is the resulting molarity?

Here it's saying if 920 ml's of water is added to 78 ml's of a 1.28 molar per bromic acid solution, what is the resulting molarity? All right. Here we're given our first molarity which we'll say is m1 and they're asking me to find the resulting molarity. So they're really asking me to find m2. And if this is m1 and of means multiply, that would mean that this has to be v1. So we're going to use a dilution equation, m1v1 equals m2v2. So that's going to be 1.28 molar. We have 78 ml's. We don't know what our resulting molarity is, so that's m2. Remember, we said up above that v2 represents our final volume. V2 represents v1 plus the volume of water added. So the initial volume we had was 78 ml's and we added another 920 ml's of water to that. So it's going to be 998 ml's for my V2. Here we can keep the units in milliliters for both the volumes because they're going to cancel out. The ml's here cancel out, so my m2 comes out to being 0 point 100 molar as my new concentration for my solution after the addition of 920 ml of water. Remember, when we're dealing with a dilution, we're just simply adding water to a concentrated solution to get a new lower concentration at the end. So take keep in mind some of the techniques we used here as we continue our exploration of dilutions.

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1. Chemical Measurements1h 50m
2. Tools of the Trade1h 17m
3. Experimental Error1h 52m
4 & 5. Statistics, Quality Assurance and Calibration Methods1h 57m
6. Chemical Equilibrium3h 41m
7. Activity and the Systematic Treatment of Equilibrium1h 0m
8. Monoprotic Acid-Base Equilibria1h 53m
9. Polyprotic Acid-Base Equilibria2h 17m
10. Acid-Base Titrations2h 37m
11. EDTA Titrations1h 34m
12. Advanced Topics in Equilibrium1h 16m
13. Fundamentals of Electrochemistry2h 19m
14. Electrodes and Potentiometry41m
15. Redox Titrations1h 14m
16. Electroanalytical Techniques57m
17. Fundamentals of Spectrophotometry50m

1. Chemical Measurements

Volumetric Analysis

Analytical Chemistry

1. Chemical Measurements

Volumetric Analysis

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Multiple Choice

If 920 mL of water is added to 78.0 mL of a 1.28 M HBrO₄ solution what is the resulting molarity?

0.110 M

15.1 M

0.100 M

0.119 M

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Verified step by step guidance

First, calculate the initial number of moles of HBrO4 in the solution using the formula: \( \text{moles} = \text{molarity} \times \text{volume in liters} \). Convert 78.0 mL to liters by dividing by 1000.

Use the initial molarity (1.28 M) and the converted volume (0.078 L) to find the moles of HBrO4: \( \text{moles of HBrO4} = 1.28 \times 0.078 \).

Next, determine the total volume of the solution after adding water. Add the initial volume of the HBrO4 solution (78.0 mL) to the volume of water added (920 mL) to get the total volume in mL, then convert this total volume to liters.

Calculate the resulting molarity of the solution using the formula: \( \text{molarity} = \frac{\text{moles of solute}}{\text{total volume in liters}} \). Use the moles calculated in step 2 and the total volume in liters from step 3.

Finally, simplify the expression to find the resulting molarity of the solution. This will give you the concentration of HBrO4 after dilution.