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Olegator [25]
3 years ago
12

3. How many moles of H20 are in 15.2 grams of pure ice?

Chemistry
1 answer:
inna [77]3 years ago
7 0

Answer:

18.01528 grams.

Explanation:

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Determine the acid dissociation constant for a 0.0250 M weak acid solution that has a pH of 2.37 . The equilibrium equation of i
Oksanka [162]

Answer:

For part (a): pHsol=2.22

Explanation:

I will show you how to solve part (a), so that you can use this example to solve part (b) on your own.

So, you're dealing with formic acid, HCOOH, a weak acid that does not dissociate completely in aqueous solution. This means that an equilibrium will be established between the unionized and ionized forms of the acid.

You can use an ICE table and the initial concentration ofthe acid to determine the concentrations of the conjugate base and of the hydronium ions tha are produced when the acid ionizes

HCOOH(aq]+H2O(l]⇌ HCOO−(aq] + H3O+(aq]

I 0.20 0 0

C (−x) (+x) (+x)

E (0.20−x) x x

You need to use the acid's pKa to determine its acid dissociation constant, Ka, which is equal to

3 0
2 years ago
Match these items.
notka56 [123]
Litmus is an indicator
Charged particles are ions
Acids contain H+ ions
Bases contain OH - ions
Hydronium ions are H3O+

Now, I have to take issue with the last one
A base of pH 14 is not a strong base, it would be a highly concentrated base. A strong base is a base that completely deionizes in water.

But technically, for the purpose of your answer strong base = pH 14
6 0
2 years ago
Calculate the energy E of a sample of 3.50 mol of ideal oxygen gas (O2) molecules at a temperature of 310 K. Assume that the mol
love history [14]

Answer:

13.53 kJ

Explanation:

The energy of a gas can be calculated by the equation:

E = (3/2)*n*R*T

Where n is the number of moles, R is the gas constant (8.314 J/mol.K), and T is the temperature.

E = (3/2)*3.5*8.314*310

E = 13,531.035 J

E = 13.53 kJ

7 0
2 years ago
How many grams of water will form if 10.54 g H2 react with 95.10 g O2?
sergeinik [125]

Answer:

94.0

Explanation:

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7 0
3 years ago
What volume of a 0.155 M potassium hydroxide solution is required to neutralize 25.7 mL of a 0.388 M hydrobromic acid solution
vekshin1

Answer: Therefore, the volume of a 0.155 M potassium hydroxide solution  is 56.0 ml

Explanation:

Molarity of a solution is defined as the number of moles of solute dissolved per Liter of the solution.

According to the neutralization law,

n_1M_1V_1=n_2M_2V_2

where,

M_1 = molarity of HBr solution = 0.338 M

V_1 = volume of HBr solution = 25.7 ml

M_2 = molarity of KOH solution = 0.155 M

V_2 = volume of KOH solution = ?

n_1 = valency of HBr = 1

n_2 = valency of KOH = 1

1\times 0.338\times 25.7=1\times 0.155\times V_2

V_2=56.0ml

Therefore, the volume of a 0.155 M potassium hydroxide solution  is 56.0 ml

8 0
2 years ago
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