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Bingel [31]
3 years ago
10

25.0 mL of an HBr solution were titrated with 29.15 mL of a 0.205 M LiOH solution to reach the equivalence point. What is the mo

larity of the HBr solution?
Chemistry
1 answer:
trapecia [35]3 years ago
7 0

The molarity of HBr solution is 0.239 M

calculation

write the equation for reaction

that is LiOH +HBr → LiBr +H20

find the moles of LiOH used

moles =molarity x volume

=0.205 x 29.15 = 5.976 moles

by use of mole ratio between LiOH :HBr which is 1:1 the moles of HBr is therefore= 5.976 moles

Molarity of HCL= moles /volume

= 5.976/25 = 0.239 M

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Consider the insoluble compound nickel(II) hydroxide , Ni(OH)2 . The nickel ion also forms a complex with cyanide ions . Write a
natali 33 [55]

Answer: Equilibrium constant for this reaction is 2.8 \times 10^{15}.

Explanation:

Chemical reaction equation for the formation of nickel cyanide complex is as follows.

Ni(OH)_{2}(s) + 4CN^{-}(aq) \rightleftharpoons [Ni(CN)_{4}^{2-}](aq) + 2OH^{-}(aq)

We know that,

      K = K_{f} \times K_{sp}

We are given that, K_{f} = 1.0 \times 10^{31}

and,    K_{sp} = 2.8 \times 10^{-16}

Hence, we will calculate the value of K as follows.

     K = K_{f} \times K_{sp}

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        = 2.8 \times 10^{15}

Thus, we can conclude that equilibrium constant for this reaction is 2.8 \times 10^{15}.

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3 years ago
**PLATO QUESTION, PLEASE ANSWER CORRECTLY**
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The corect answers will be:
1) A
2) B
3) D

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