Question

In: Chemistry

Determine each of the following for a 0.170 M HBr solution: A.[H3O+] B.pH C.pOH D.Write the...

Determine each of the following for a 0.170 M HBr solution:

A.[H3O+]

B.pH

C.pOH

D.Write the balanced equation for the reaction with LiOH.

E. Calculate the volume, in milliliters, of HBr solution required to neutralize 46.0 mL of a 0.160 M LiOH solution .

Expert Solution

(A) We have 0.170 M HBr solution. The dissociation of HBr is

So concentration of H+ ion, [] = 0.170 M

Also

Therefore the concentration of H3O+ , = 0.170 M

(B) pH of the HBr solution is,

(C) pOH of the solution is

(D) The reaction between HBr(acid) and LiOH(basic) results in LiBr(salt) and H2O balanced chemical equation of reaction between HBr and LiOH solution,

(E) We have the neutralization reaction,

We have the Molarity of HBr (M1) = 0.170M

Volume of the HBr solution (V1) =??

Molarity of LiBr solution (M2) = 0.160 M

Volume of LiBr solution (V2) = 46.0 mL

We can calculate the volume of HBr solution by using dilution law,

Volume of HBr requires to neutralise the LiOH solution,

V1 = 43.3 mL

queen_honey_blossom answered 2 years ago

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