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4 years ago

What is the [H30+) in a solution with (OH'] = 2.0 x 10-3 m?

Chemistry

1 answer:

Nezavi [6.7K]4 years ago

8 0

Answer: 5.0 x 10-12 M

Explanation:

It is well known that; pH + pOH = 14.

pOH = - log [ OH-]

= - log [ 2.0 x 10 ∧-3]

= 3 - log 2

= 3 - 0.301 = 2.7 approximately.

recall that, pH + pOH = 14, therefore; pH = 14 - 2.7 = 11.3

pH = - log [ H3O+]

11.3 = - log [H3O+], take the antilog of 11.3, gives us;

[H3O+] = antilog of - 11.3, which gives 5.0 x 10-12 M

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Convert 1663.5 g to mg

WINSTONCH [101]

Answer:

It will be 1663500mg

Explanation:

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4 years ago

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How many moles of KCl are contained in this solution?<br><br>0.486 L of a 2.0 M KCl solution

Vika [28.1K]

Answer:

0.972mol

Explanation:

Given parameters:

Volume of Solution of KCl = 0.486L

Molarity = 2.0M

Unknown:

Number of moles of KCl in solution = ?

Solution:

To find the number of moles of KCl in this solution, use the expression below;

Number of moles = molarity x volume

Insert the parameters and solve;

Number of moles = 0.486 x 2 = 0.972mol

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3 years ago

Two liquids are combined and a gas is released is this a chemical change?

marshall27 [118]

Answer:

yes it is a chemical change

Explanation:

because first it was in liquid and turned into gas

6 0

3 years ago

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Given the following information:Br2 bond energy = 193 kJ/mol F2 bond energy = 154 kJ/mol 1/2Br2(g) + 3/2F2(g) -> BrF3(g) = –3

arlik [135]

Answer:

C) 712 KJ/mol

Explanation:

ΔH°r = Σ Eb broken - Σ Eb formed

1/2Br2(g) + 3/2F2(g) → BrF3(g)

∴ ΔH°r = - 384 KJ/mol

∴ Br2 Eb = 193 KJ/mol

∴ F2 Eb = 154 KJ/mol

⇒ Σ Eb broken = (1/2)(Br-Br) + (3/2)(F-F)

⇒ Σ Eb broken = (1/2)(193 KJ/mol) + (3/2)(154 KJ/mol) = 327.5 KJ/mol

∴ Eb formed: Br-F

⇒ Σ Eb formed (Br-F) = Σ Eb broken - ΔH°r

⇒ Eb (Br-F) = 327.5 KJ/mol - ( - 384 KJ/mol )

⇒ Eb Br-F = 327.5 KJ/mol + 384 KJ/mol = 711.5 KJ/mol ≅ 712 KJ/mol

8 0

3 years ago

Magnesium metal (0.100 mol) and a volume of aqueous hydrochloric acid that contains 0.500 mol of HCl are combined and react to c

jok3333 [9.3K]

Answer:

2.24 L of hydrogen gas, measured at STP, are produced.

Explanation:

Given, Moles of magnesium metal, $Mg$ = 0.100 mol

Moles of hydrochloric acid, $HCl$ = 0.500 mol

According to the reaction shown below:-

$Mg_{(s)} + 2HCl_{(aq)}\rightarrow MgCl_2_{(aq)} + H_2_{(g)}$

1 mole of Mg reacts with 2 moles of $HCl$

0.100 mol of Mg reacts with 2*0.100 mol of $HCl$

Moles of $HCl$ must react = 0.200 mol

Available moles of $HCl$ = 0.500 moles

Limiting reagent is the one which is present in small amount. Thus, $Mg$ is limiting reagent.

The formation of the product is governed by the limiting reagent. So,

1 mole of $Mg$ on reaction forms 1 mole of $H_2$

0.100 mole of $Mg$ on reaction forms 0.100 mole of $H_2$

Mole of $H_2$ = 0.100 mol

At STP,

Pressure = 1 atm

Temperature = 273.15 K

Volume = ?

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:

1 atm × V L = 0.100 × 0.0821 L.atm/K.mol × 273.15 K

2.24 L of hydrogen gas, measured at STP, are produced.

4 0

3 years ago