A 0.100 M solution of HBrO has a pH of 4.843. Find the Ka...

Transcript

0:00 Hi all.

00:02 So we have this question over here which is 0 .10.

00:06 M of hbro solution right.

00:10 It is going to have this concentration.

00:12 The ph of that solution is 4 .843.

00:15 We want to find out the k of the given solution.

00:19 Right.

00:20 So first let us write out the formula for the ka which is ka will be equal to h3oi .n.

00:29 Right? the union.

00:31 The whole divided by a solution which is h a fine this is the formula which we are going to use and this is something which we have to remember fine okay so now we are going to start off we have this concentration of the given solution let us first write down the dissociation reaction of this solution fine so hbro it is going to dissociate into we have your bro minus in aqueous obviously plus we will have h3o the hydrogen ion right in aquis also so now this is our reaction this will have to use the ice rule in this first step to find out the concentrations fine so we'll have used the ice rule the first is i that is initial concentration second is c which is the change in the concentration and last is the e which is the equilibrium fine so at initial initially the constant is given to us which is 0 .1 for hb r o it is going to get dissociated so these products have not yet formed at initial point right so it is going to be zero and zero right so now this whole thing it is going to get dissociated into these two ions over here so we'll consider x to be the concentration if we consider x to be these concentrations over here like this x x and x we are going to write it equivalently because these ions are going to get dissociated equally right there is no coefficient of here so x and x so it is going to be since this is going to get depleted we are going to write it as minus x and they are going to be formed now but in what amount they are formed we do not know so it is going to be x and x right so now at equilibrium the concentration will be initial minus the change so it is going to be 0 .1 minus x right and then we have the products as well which is will be which will remain x as well so this is what we have found out fine according to the ice so the next step what we are going to do is the ph is given to us already so with the help of ph we'll try to find out the concentration of the h3 o plus ion so we know that minus ph it is going to be equal to the log of the concentration of h3o plus iron fine ph value is given to us which is minus 4 .843 we are going to just go in the formula so now h3 o plus it is going to become 10 raised 2 minus 4 .843 when we solve this will get the answer which is 1 .485 into 10 raised to minus 5 this is the value of our x which we have written over here fine so now we have found out the value of x now all we have to do is simply use the formula of the k which we previously wrote which we wrote at the very start and then we can write of the answer...

Question

A 0.100 M solution of HBrO has a pH of 4.843. Find the Ka for HBrO.

Question

A 0.100 M solution of HBrO has a pH of 4.843. Find the Ka for HBrO.

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