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3 years ago

A solution containing an equal number of hydrogen ions and hydroxide ions isA. basicB. alkalineC. acidicD. neutral.

Chemistry

1 answer:

Goryan [66]3 years ago

5 0

Answer:

Neutral (Option D)

Explanation:

[H₃O⁺] = [OH⁻] → Neutral solution pH = 7

[H₃O⁺] < [OH⁻] → Alkaline / Basic solution pH > 7

[H₃O⁺] > [OH⁻] → Acidic solution pH < 7

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What is AgNO3 + KCI-KNO3+AgCI. What type of reaction does this represent

PIT_PIT [208]

<span>C4H10 + 6.5 O2 ----> 4CO2 + 5H2O

2C4H10 + 13 O2 ----> 8CO2 + 10H2O

1. Count the C on the left (4), put a 4 where the C on the right.

2. Count the H on the left (1), you have two on the right, so you multimply this two by 5. Put the 5 in front of the H2O

3. Count the O on the right. You have 4*2 + 5 = 13. You have two on the left, so you need 6.5 on the left.

4. Now multiply everything on the equation by two so you have nice integer numbers.

5. check you have the same amount of everything on each side.
Example C: left 8, right 8, etc.
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6 0

3 years ago

PLEASE HELPPP!!!!!!!!

Stells [14]

Explanation:

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Label B: oceanic - continental

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3 years ago

Read 2 more answers

If the pressure on a 1.04 L sample of gas is doubled at constant temperature, please compute the new volume of gas: __

natulia [17]

Answer:

0.52 L.

Explanation:

Let P be the initial pressure.

From the question given above, the following data were obtained:

Initial pressure (P1) = P

Initial volume (V1) = 1.04 L

Final pressure (P2) = double the initial pressure = 2P

Final volume (V2) =?

The new volume (V2) of the gas can be obtained by using the the Boyle's law equation as shown below:

P1V1 = P2V2

P × 1.04 = 2P × V2

1.04P = 2P × V2

Divide both side by 2P

V2 = 1.04P /2P

V2 = 0.52 L

Thus, the new volume of the gas is 0.52 L.

6 0

3 years ago

Can someone help? I wasn't at school the day we did this and I don't understand.

Anton [14]

1) 2700 kg/l
2) 13.6 kg/l
3) 0.1578 kg
4) 8921.5 kg/m3
5) 1.59 kg/l
6) 1.84 kg/l
7) 0.21965 kg
8) 11331.9 kg/m3
9) 7.9167 kg/l
10) 238.095 cm3

Just divide the masses by volume to find out the density, multiply the volume with density to find out the mass and divide the mass by density to find out the volume.
To turn the result into SI unit (kg/l), divide the g by 1000 and ml by 1000.

7 0

4 years ago

What is the molar mass of a gas if a flask with a volume of 3. 16 l contains 9. 33 grams of the gas at 32. 0°c and 1. 00 atm?

Serhud [2]

The molar mass of a gas if a flask with a volume of 3. 16 L contains 9. 33 grams of the gas at 32. 0°C and 1. 00 atm is 1.17g/mol

Calculation ,

In this question we have to fist find the number of moles of gas by using ideal gas equation and from the help of number of moles we can determine molar mass.

According to ideal gas equation which is also known as ideal law ,

PV = nRT ...( i )

where P is the pressure of the gas = 1 atm

V is the volume of the gas in the flask with volume = 3. 16 L

R is the universal gas constant = 0.082 atm L/K mol

T is the temperature = 32. 0°C = 32 + 273 = 305 K

n is the number of moles = ?

Putting the value of Pressure P , volume V , temperature T , number of moles n and universal gas constant R in the equation (i) we get ,

1 atm ×3. 16 L = n× 0.082 atm L/K mol ×305 K

n = 1 atm ×3. 16 L / 0.082 atm L/K mol × 305 K = 0.126 mole

number of mole of a gas = 0.126 mole = given mass/ molar mass

molar mass = number of moles × Given mass = 0.126 × 9. 33 = 1.17g/mol

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1 year ago