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3 years ago

How does H3PO ionize in water ?

Chemistry

1 answer:

Nonamiya [84]3 years ago

5 0

Answer:

H3PO4 + H2O ↔ $H^{+}$ + $H2PO4^{-}$

Explanation:

HNO3 → NO2 + H2O + O2

H2SO4 → SO3 + H2O + O2

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Which composer made it a goal to create compositions that sounded truly american?.

MAVERICK [17]

Given what we know, we can confirm that the composer who made it a goal to create compositions that sounded truly American was Aaron Copland.

<h3>Who was Aaron Copland?</h3>

Aaron Copland was an American composer, among his other disciplines, best known for his jazz-styled music. He went on to win an Oscar award for film composing for the movie The Heiress (1949).

Therefore, we can confirm that the composer who made it a goal to create compositions that sounded truly American was Aaron Copland.

To learn more about music visit:

brainly.com/question/8051042?referrer=searchResults

7 0

3 years ago

a chemist dissolves 0.564 moles of manganese (IV) oxide (MnO2) in water, and adds enough water to make 0.510 L of solution. Calc

ladessa [460]

Answer:

The molarity of the solution is 1.1 $\frac{moles}{liter}$

Explanation:

Molarity is a measure of the concentration of that substance that is defined as the number of moles of solute divided by the volume of the solution.

The molarity of a solution is calculated by dividing the moles of the solute by the volume of the solution:

$molarity=\frac{number of moles of solute}{volume}$

Molarity is expressed in units $\frac{moles}{liter}$

In this case

number of moles of solute= 0.564 moles
volume= 0.510 L

Replacing:

$molarity=\frac{0.564 moles}{0.510 L}$

Solving:

molarity= 1.1 $\frac{moles}{liter}$

The molarity of the solution is 1.1 $\frac{moles}{liter}$

4 0

3 years ago

A 25.0 liter rigid container has a mixture of 32.00 grams of oxygen gas and 1 point

Ksivusya [100]

Answer:

$P_{T}$ = 2.94 atm

Explanation:

The total pressure ( $P_{T}$ ) in the container is given by:

$P_{T} = P_{O_{2}} + P_{He}$

The pressure of the oxygen ( $P_{O_{2}}$ ) and the pressure of the helium ( $P_{He}$ ) can be calculated using the ideal gas law:

$PV = nRT$

Where:

V: is the volume = 25.0 L

n: is the number of moles of the gases

R: is the gas constant = 0.082 Latm/(Kmol)

T: is the temperature = 298 K

First, we need to find the number of moles of the oxygen and the helium:

$n_{O_{2}} = \frac{m}{M}$

Where m is the mass of the gas and M is the molar mass

$n_{O_{2}} = \frac{32.00 g}{31.998 g/mol} = 1.00 moles$

And the number of moles of helium is:

$n_{He} = \frac{8.00 g}{4.0026 g/mol} = 2.00 moles$

Now, we can find the pressure of the oxygen and the pressure of the helium:

$P_{O_{2}} = \frac{nRT}{V} = \frac{1.00 moles*0.082 Latm/(Kmol)*298 K}{25.0 L} = 0.98 atm$

$P_{He} = \frac{nRT}{V} = \frac{2.00 moles*0.082 Latm/(Kmol)*298 K}{25.0 L} = 1.96 atm$

Finally, the total pressure in the container is:

$P_{T} = P_{O_{2}} + P_{He} = 0.98 atm + 1.96 atm = 2.94 atm$

Therefore, the total pressure in the container is 2.94 atm.

I hope it helps you!

6 0

4 years ago

How does meiosis help in creating genetic diversity?

mezya [45]

Creating individually unique cells

5 0

3 years ago

Read 2 more answers

How many grams of testosterone, C19H28O2 (288.4 g/mol), must be dissolved in 299.0 grams of benzene to reduce the freezing point

iVinArrow [24]

Answer: 8.42 grams of testosterone

Explanation:

Depression in freezing point is given by:

$\Delta T_f=i\times K_f\times m$

$\Delta T_f=0.500^0C$ = Depression in freezing point

i= vant hoff factor = 1 (for non electrolyte)

$K_f$ = freezing point constant of benzene= $5.12^0C/m$

m= molality

$\Delta T_f=i\times K_f\times \frac{\text{mass of solute}}{\text{molar mass of solute}\times \text{weight of solvent in kg}}$

Weight of solvent (benzene)= 299.0 g = 0.299 kg

Molar mass of solute testosterone= 288.4 g/mol

Mass of solute testosterone added = ?

$0.500=1\times 5.12\times \frac{xg}{288.4 g/mol\times 0.299kg}$

$x=8.42g$

Thus 8.42 grams of testosterone must be dissolved in 299.0 grams of benzene to reduce the freezing point by 0.500°C.

8 0

4 years ago