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3 years ago

Need help filling the blanks here ! Titration of Acids and Bases with given data .Chemistry

Chemistry

1 answer:

MissTica3 years ago

6 0

Answer:

DONT KNOW BUDDY O WELL

Explanation:

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What type of heat transfer warms our oceans and atmosphere

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4 years ago

How many grams is .15mol of argon

bonufazy [111]

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The answer is 39.948.

Explanation:

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3 years ago

A compound was found to be soluble in water. It was also found that addition of acid to an aqueous solution of this compound res

gogolik [260]

Answer:

c. Cr

Explanation:

$Cr^3+(aq) + CO_3^2-(aq) ------------> Cr_2CO_3(s)$

The compound is containing $CO_3^2-$ ion.

If acid reacts with it, CO_2 evolves.

$H^+ + CO_3^2- ----------> H_2O + CO_2$

therefore, Cr would form a precipitate when added to an aqueous solution of this compound. Cr2CO3 is the precipitate.

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3 years ago

When 6.040 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 18.95 grams of CO2 and 7.759 grams of H

algol [13]

Answer: The empirical formula is $CH_2$ and molecular formula is $C_4H_8$

Explanation:

We are given:

Mass of $CO_2$ = 18.95 g

Mass of $H_2O$ = 7.759 g

Molar mass of carbon dioxide = 44 g/mol

Molar mass of water = 18 g/mol

For calculating the mass of carbon:

In 44g of carbon dioxide, 12 g of carbon is contained.

So, in 18.59 g of carbon dioxide, = $\frac{12}{44}\times 18.59=5.07g$ of carbon will be contained.

For calculating the mass of hydrogen:

In 18g of water, 2 g of hydrogen is contained.

So, in 7.759 g of water, = $\frac{2}{18}\times 7.759=0.862g$ of hydrogen will be contained.

Mass of C = 5.07 g

Mass of H = 0.862 g

Step 1 : convert given masses into moles.

Moles of C = $\frac{\text{ given mass of C}}{\text{ molar mass of C}}= \frac{5.07g}{12g/mole}=0.422moles$

Moles of H= $\frac{\text{ given mass of H}}{\text{ molar mass of H}}= \frac{0.862g}{1g/mole}=0.862moles$

Step 2 : For the mole ratio, divide each value of moles by the smallest number of moles calculated.

For C = $\frac{0.422}{0.422}=1$

For H = $\frac{0.862}{0.422}=2$

The ratio of C : H = 1: 2

Hence the empirical formula is $CH_2$ .

The empirical weight of $CH_2$ = 1(12)+2(1)= 14 g.

The molecular weight = 56.1 g/mole

Now we have to calculate the molecular formula.

$n=\frac{\text{Molecular weight }}{\text{Equivalent weight}}=\frac{56.1}{14}=4$

The molecular formula will be= $4\times CH_2=C_4H_8$

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3 years ago

What is The maximum amount of a substance that can be dissolved by another substance

Oksanka [162]

Solubility varies vastly. It depends on the solute, solvent, temperature, and pressure.

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3 years ago