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3 years ago

What is the pOH of a solution that has a pH of 2

Chemistry

1 answer:

olga nikolaevna [1]3 years ago

5 0

POH is 12.
Explanation:
The pOH + pH has to equal 14
Since we know pH, you do:
pOH = 14-pH
pOH = 14-2
pOH = 12

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How many moles are in 124.7 g of Ba(OH)2

Alekssandra [29.7K]

Answer:

0.73 mol

Explanation:

No. of moles(n)= Given mass/molar mass.

Given mass=124.7g

Molar mass of Ba(OH)2= Molar mass of (Barium+2Oxygen+2Hydrogen)=137+32+2=171g

No. of moles= 124.7g/171g=0.73 mol

7 0

3 years ago

A 3.00-L flask is filled with gaseous ammonia, NH3. The gas pressure measured at 27.0 ∘C is 2.55 atm . Assuming ideal gas behavi

Whitepunk [10]

Answer : The mass of ammonia present in the flask in three significant figures are, 5.28 grams.

Solution :

Using ideal gas equation,

$PV=nRT\\\\PV=\frac{w}{M}\times RT$

where,

n = number of moles of gas

w = mass of ammonia gas = ?

P = pressure of the ammonia gas = 2.55 atm

T = temperature of the ammonia gas = $27^oC=273+27=300K$

M = molar mass of ammonia gas = 17 g/mole

R = gas constant = 0.0821 L.atm/mole.K

V = volume of ammonia gas = 3.00 L

Now put all the given values in the above equation, we get the mass of ammonia gas.

$(2.55atm)\times (3.00L)=\frac{w}{17g/mole}\times (0.0821L.atm/mole.K)\times (300K)$

$w=5.28g$

Therefore, the mass of ammonia present in the flask in three significant figures are, 5.28 grams.

8 0

4 years ago

By making several measurements with the same balance, a chemist obtained values of 5.224 g, 5.235 g, and 5.259 g for the mass of

stepan [7]

Answer:

a) Measurements have a good precision.

Explanation:

Accuracy is the proximity of the data to the value considered as real, in this situation we do not know the real value and we do not know if the data is accurate or not, so we can discard options b and d.

Now, precision is the proximity of the data obtained among themselves and that is what we can observe, so the appropriate answer is the option a.

6 0

3 years ago

A balloon is filled with 0.250 mole of air at 35Â°C. If the volume of the balloon is 6.23 liters, what is the absolute pressure

lord [1]

Answer is: the absolute pressure of the air in the balloon is 1.015 atm (102.84 kPa).

n = 0.250 mol; amount of substance.

V = 6.23 L; volume of the balloon.

T = 35°C = 308.15 K; temperature.

R = 0.08206 L·atm/mol·K, universal gas constant.

Ideal gas law: p·V = n·R·T.

p = n·R·T / V.

p = 0.250 mol · 0.08206 L·atm/mol·K · 308.15 K / 6.23 L.

p = 1.015 atm; presure of the air.

6 0

3 years ago

The object is traveling at a velocity of m/s.

marishachu [46]

Answer:

$= 3.75m {s}^{ - 1} \\$

Explanation:

$velocity = \frac{displacement}{time} \\ = \frac{15m}{4s} \\ = 3.75m {s}^{ - 1}$

3 0

4 years ago