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3 years ago

What solvent should you use to measure the density of naphthalene acid?

1 answer:

3 0

Water b/c it is insoluble in water. it is soluble in cyclohexane and sparingly <span>soluble in ethyl alcohol.

Hope this helps</span>

You might be interested in

how many coefficients need to be changed to make this chemical equation balanced? Zn + HNO3 --> Zn (No3)2 + H2

mestny [16]

Coefficient 2 should be placed in the equation before the nitric acid in the reactant so that the chemical reaction becomes balanced.

The given chemical reaction is,

Zn + HNO3 --------> Zn (No3)2 + H2

Here, the elements Hydrogen, Nitrogen, and Oxygen are unbalanced.

These elements are altogether found in HNO₃ on the reactant side and are found as nitrate and hydrogen gas on the product side.

To balance the equation, the coefficient 2 is to be added in the reactant side so that 2 moles of Hydrogen, Nitrogen, and Oxygen would be balanced with 2 moles of Nitrate and two moles of Nitrogen.

On adding 2 on reactant side, we get

Zn + 2HNO3 -----------> Zn(NO3)₂ + H₂

This gives us a balanced equation and thus the equation could be balanced this way.

Therefore, coefficient 2 is to be added to make the equation to be balanced.

To know more about the balanced equation, click below:

brainly.com/question/26694427

#SPJ1

8 0

1 year ago

How are owls compared to wolfs?

xenn [34]

Answer:

They are both very aggressive animals! And amazing hunters at night!

Explanation:

I hope this helps! :)

6 0

2 years ago

Read 2 more answers

WHAT MASS OF 1,1 DICHLOROEHTANE MUST BE MIXED WITH 100G OF 1,1 DICHLOROTETRAFLUOROEHTANE TO GIVE A SOLUTION WITH VAPOR PRESSURE

vaieri [72.5K]

This is an incomplete question.

The complete question is:

1,1-dichlorotetrafluoroethane, CF3CCL2F, has a vapor pressure of 228 torr. What mass of 1,1-dichloroethane must be mixed with 100.0 g of 1,1-dichlorotetrafluoroethane to give a solution with vapor pressure 157 torr at 25 degrees celsius?

Answer: 46.9 g of 1,1 dichloroethane must be fixed with 100 g of 1,1 dichlorotetrafluoroethane to give a solution with vapor pressure of 157 torr at $25^0C$

Explanation:

As the relative lowering of vapor pressure is directly proportional to the amount of dissolved solute.

The formula for relative lowering of vapor pressure will be,

$\frac{p^o-p_s}{p^o}=i\times x_2$

where,

$\frac{p^o-p_s}{p^o}$ = relative lowering in vapor pressure

i = Van'T Hoff factor = 1 (for non electrolytes)

$x_2$ = mole fraction of solute

= $\frac{\text {moles of solute}}{\text {total moles}}$

Given : x g of solute is present in 100 g of solvent

moles of solute (1,1 DICHLOROEHTANE) = $\frac{\text{Given mass}}{\text {Molar mass}}=\frac{xg}{98.96g/mol}moles$

moles of solvent (1,1 DICHLOROTETRAFLUOROEHTANE ) = $\frac{\text{Given mass}}{\text {Molar mass}}=\frac{100g}{170.92g/mol}=0.58moles$

Total moles = moles of solute + moles of solvent = $\frac{xg}{98.96g/mol}+0.58$

$x_2$ = mole fraction of solute = $\frac{\frac{xg}{98.96g/mol}}{\frac{xg}{98.96g/mol}+0.58}$

$\frac{228-157}{157}=1\times \frac{\frac{xg}{98.96g/mol}}{\frac{xg}{98.96g/mol}+0.58}$

$0.45=1\times \frac{\frac{xg}{98.96g/mol}}{\frac{xg}{98.96g/mol}+0.58}$

$x=46.9g$

Thus 46.9 g of 1,1 dichloroethane must be fixed with 100 g of 1,1 dichlorotetrafluoroethane to give a solution with vapor pressure of 157 torr at $25^0C$

5 0

4 years ago

A 17.6-g sample of ammonium carbonate contains ________ mol of ammonium ions.

postnew [5]

These problems are a bit interesting. :)

First let's write the molecular formula for ammonium carbonate.

NH4CO3 (Note! The 4 and 3 are subscripts, and not coefficients)

17.6 gNH4CO3

Now to convert to mol of one of our substances we take the percent composition of that particular part of the molecule and multiply it by our starting mass. This is what it looks like using dimensional analyse.

17.6 gNH4CO3 * (Molar Mass of NH4 / Molar Mass of NH4CO3)

Grab a periodic table (or look one up) and find the molar masses for these molecules! Well. In this case I'll do it for you. (Note: I round the molar masses off to two decimal places)

NH4 = 14.01 + 4*1.01 = 18.05 g/mol
NH4CO3 = 14.01 + 4*1.01 + 12.01 + 3*16.00 = 78.06 g/mol

17.6 gNH4CO3 * (18.05 molNH4 / 78.06 molNH4CO3)
= 4.07 gNH4

Now just take the molar mass we found to convert that amount into moles!

4.07 gNH4 * (1 molNH4 / 18.05 gNH4) = 0.225 molNH4

4 0

3 years ago

Are any of the bonds formed between the following pairs of atoms ionic?

melamori03 [73]

Answer:

O and H

Explanation:

I don't know the explanation

5 0

3 years ago