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Natali [406]
3 years ago
15

How many grams of water can be produced when 65.5 grams of sodium hydroxide reacts with excess sulfuric acid? (4 points) You mus

t balance this equation first! H2SO4 + NaOH → H2O + Na2SO4 Show, or explain, all of your work along with the final answer.
Chemistry
1 answer:
stiks02 [169]3 years ago
5 0
Balanced Equation: H2SO4 + 2NaOH --> 2H2O + Na2SO4

Moles= Mass/RMM
= 65.5/40
= 1.6375

Mole Ratio = 2:2
= 1.6375

Mass (H2O) = 1.64 x 18
= 29.5 g
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In the titration of wine to determine the acid concentration, 10.0 mL of wine was placed in a beaker and diluted with 40.0 mL of
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Answer:

0.0042 M is the molarity of tartaric acid in this sample of wine.

Explanation:

To calculate the concentration of acid, we use the equation given by neutralization reaction:

n_1M_1V_1=n_2M_2V_2

where,

n_1,M_1\text{ and }V_1 are the n-factor, molarity and volume of acid which is tartaric acid

n_2,M_2\text{ and }V_2 are the n-factor, molarity and volume of base which is NaOH.

We are given:

n_1=2\\M_1=?\\V_1=10.0+40.0 mL=50.0 mL\\n_2=1\\M_2=0.051 M M\\V_2=8.20 mL

Putting values in above equation, we get:

2\times M_1\times 50.0 mL=1\times 0.051 M\times 8.20 mL

M_1=\frac{1\times 0.051 M\times 8.20 mL}{2\times 50.0 mL}=0.0042 M

0.0042 M is the molarity of tartaric acid in this sample of wine.

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Mercury has a density of 13.6 g/mL. How many milliliters of mercury have a mass of 350 g? *
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