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Sauron [17]
3 years ago
5

An acetic acid buffer solution is required to have a pH of 5.27. You have a solution that contains 0.010 mol of Acetic acid. Wha

t molarity of sodium acetate will you need to add to the solution
Chemistry
1 answer:
dlinn [17]3 years ago
7 0

Answer:

Molarity of sodium acetate you will need to add is 0.0324M

Explanation:

<em>Assuming volume of the buffer is 1L.</em>

<em />

The pH of a buffer can be determined using Henderson-Hasselbalch equation:

pH = pKa + log [A⁻] / [HA]

<em>Where pKa is pKa of the weak acid,  [A⁻] molar concentration of conjugate base and [HA] molar concentration of weak acid</em>

<em />

Replacing for the acetic buffer (pKa = 4.76):

pH = 4.76 + log [Sodium Acetate] / [Acetic Acid]

As you have 0.010 moles of acetic acid in 1L:

[Acetic Acid] = 0.010mol / 1L = 0.010M

And you require a pH of 5.27:

5.27 = 4.76 + log [Sodium Acetate] / [0.010M]

0.51 = log [Sodium Acetate] / [0.010M]

10^0.51 = [Sodium Acetate] / [0.010M]

3.236 =  [Sodium Acetate] / [0.010M]

3.236 [0.010M] = [Sodium Acetate]

0.0324M = [Sodium Acetate]

<h3>Molarity of sodium acetate you will need to add is 0.0324M</h3>

<em />

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How many moles of Mg(OH)2(aq) would be required to neutralize 6.0 mol HCl(aq)?
jekas [21]

Answer:

3.0molMg(OH)_2

Explanation:

Hello there!

In this case, for these types of acid-base neutralizations, it is crucial to firstly set up the chemical reaction taking place between the acid and the base; in this case HCl and Mg(OH)2 respectively, whose products are obtained by switching around the anions and cations as shown below:

HCl(aq)+Mg(OH)_2(aq)\rightarrow MgCl_2(aq)+H_2O(l)

Which must be balanced to accurately predict the mole ratio on the reactants side:

2HCl(aq)+Mg(OH)_2(aq)\rightarrow MgCl_2(aq)+2H_2O(l)

Whereas we can see a 2:1 mole ratio of the acid to the base; thus, the moles of Mg(OH) required for the neutralization of 6.0 moles of HCl turn out to be:

6.0molHCl*\frac{1molMg(OH)_2}{2molHCl} \\\\=3.0molMg(OH)_2

Best regards!

5 0
3 years ago
In a titration, 45.0 mL of KOH is neutralized by 75.0 mL of 0.30M HBr. How much KOH is in 1.0 liter of the KOH solution ?
photoshop1234 [79]
KOH + HBr ---> KBr + H2O

0,3 moles of HBr ---in-------1000ml
x moles of HBr-------in------75ml
x = 0,0225 moles of HBr

according to the reaction:  1 mole of KOH = 1 mole of HBr
so
0,0225 moles of HBr = 0,0225 moles of KOH

0,0225 mole of KOH------in-----45ml
x moles of KOH -----------in------1000ml
x = 0,5 moles of KOH

answer: 0,5 mol/dm³  KOH (molarity)


8 0
3 years ago
The compound KOH is called
denis-greek [22]

Answer:

It is called Potassium Hydroxide

4 0
3 years ago
Read 2 more answers
Using the same sample of gas (P1 = 565 torr , T1 = 27 ∘C ), we wish to change the pressure to 5650 torr with no accompanying cha
Stels [109]

Answer:

2726.85 °C

Explanation:

Given data:

Initial pressure = 565 torr

Initial temperature = 27°C

Final temperature = ?

Final pressure = 5650 torr

Solution:

Initial temperature = 27°C (27+273 = 300 K)

According to Gay-Lussac Law,

The pressure of given amount of a gas is directly proportional to its temperature at constant volume and number of moles.

Mathematical relationship:

P₁/T₁ = P₂/T₂

Now we will put the values in formula:

T₂  = P₂T₁ /P₁

T₂  = 5650 torr × 300 K / 565 torr

T₂  = 1695000 torr. K /565 torr

T₂ = 3000 K

Kelvin to degree Celsius:

3000 K - 273.15 = 2726.85 °C

4 0
2 years ago
A 25-mL solution of H2SO4 is completely neutralized by 18 mL of 1.0M NaOH. What is the concentration of the H2SO4?
Charra [1.4K]
There are several information's already given in the question. Based on the information's provided, the answer can be easily deduced.
V1 = 25 ml
     = 25/1000 liter
     = 0.025 liter
V2 = 18 ml
      = 18/1000 liter
      = 0.018 liter
M2 = 1.0 M
M1 = ?
Then
M1V1 = M2V2
M1 = M2V2/V1
      = (1 * 0.018)/0.025
      = 0.72 M
From the above deduction, it can be easily concluded that the correct option among all the options that are given in the question is the first option or option "A". I hope that this is the answer that has actually come to your help.
5 0
3 years ago
Read 2 more answers
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