What is the solubility of Na2HAsO4 at 60 degrees C

I typed a question. It said give points. I selected. Someone answered notification came. But where do I see they persons answer?

Ksivusya [100]

Answer:

212.304 grams

Explanation:

similar to your other question, use the same formula

q=mCpΔT

23617=m(4.182)(46.6-20)

23617=111.2412m

m=212.304g

6 0

1 year ago

I AM GIVING A LOT OF POINTS SO PLEASE HELP ME!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!

prohojiy [21]

Answer:c

Explanation:

it’s gained kinetic from the gravitational potential energy at the top

4 0

2 years ago

Read 2 more answers

What is the oxidation number of iodine in KL04? (1)- +1 (2)- -1 (3)- +7 (4)- -7

Nostrana [21]

3) +7

I got this stupid question wrong so that you people don't have to. I simply hate chemistry and I wish it didn't exist. Kind of like this website that makes me explain the answer.

Trust me, the answer is correct

4 0

2 years ago

1.875mps into kilometers per hour

worty [1.4K]

Answer:

6,75 kilometres per hour

6 0

2 years ago

Boron trifluoride gas is collected at 2.0 degree C in an evacuated flask with a measured volume of 15.0 L. When all the gas has

IgorC [24]

Answer:

Moles of boron trifluoride gas that were collected = 11.6 mol

Mass of boron trifluoride gas that were collected = 787 g

Explanation:

Given that:

Temperature = 2.0 °C

The conversion of T( °C) to T(K) is shown below:

T(K) = T( °C) + 273.15

So,

T = (2.0 + 273.15) K = 275.15 K

V = 15.0 L

Pressure = 0.130 atm

Using ideal gas equation as:

$PV=nRT$

where,

P is the pressure

V is the volume

n is the number of moles

T is the temperature

R is Gas constant having value = 0.0821 L atm/ K mol

Applying the equation as:

0.130 atm × 15.0 L = n ×0.0821 L atm/ K mol × 275.15 K

⇒n = 11.6 mol

Thus, Moles of boron trifluoride gas that were collected = 11.6 mol

Molar mass of boron trifluoride gas = 67.82 g/mol

The formula for the calculation of moles is shown below:

$moles = \frac{Mass\ taken}{Molar\ mass}$

Thus,

$11.6\ mole= \frac{Mass}{67.82\ g/mol}$

Mass of boron trifluoride gas that were collected = 787 g

7 0

2 years ago