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aivan3 [116]
3 years ago
7

Calculate the concentration of an aqueous solution of naoh that has a ph of 11.50

Chemistry
2 answers:
Reika [66]3 years ago
7 0
NaOH is a strong base and complete dissociation into Na⁺ and OH⁻ ions. 
Therefore [NaOH] = [OH⁻]
To calculate the [OH⁻], we can first find the pOH as NaOH is a basic solution.
pH + pOH = 14
Since pH = 11.50
pOH = 14 - 11.50
pOH = 2.50
We can calculate [OH⁻] by knowing pOH 
pOH = -log[OH⁻]
[OH⁻] = antilog(-pOH)
[OH⁻] = 3.2 x 10⁻³ M
therefore [NaOH] = 3.2 x 10⁻³ M
Alexandra [31]3 years ago
5 0
We know that;
pH + pOH = 14
Thus; pOH = 14-11.5
                  = 2.5
But; pOH = - log [OH-]
-log[OH} = 2.5
        [OH] = 10 ^-2.5
                 = 3.162 x 10^-3 M
thus; [NaOH] = 3.162 x 10^-3 M
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When 0.250 moles of KCl are added to 200.0 g of water in a constant pressure calorimeter a temperature change is observed. Given
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Explanation:

Upon dissolution of KCl heat is generated and temperature of the solution raises.

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             17.24 kJ/mol \times 0.25 mol

                = 4.31 kJ

or,             = 4310 J      (as 1 kJ = 1000 J)

Mass of solution will be the sum of mass of water and mass of KCl.

       Mass of Solution = mass of water + (no. of moles of KCl × molar mass)

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Relation between heat, mass and change in temperature is as follows.

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                     Q = mC \Delta T

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