Is A “the density of the ice decreased as it melted”
The true statement is that after reaching equilibrium, the rate of forming products and reactants is the same.
<h3>What is true about the given reaction?</h3>
The given reaction shows a reaction between A and B to form CD
The reaction is a reversible reaction.
A reversible reaction is a reaction which can proceed in either of two ways where the reactants can react to form the product and also the products an break down to form the reactants.
In the reaction given, as the concentration of A and b decreases, the concentration of CD increases and vice versa.
At equilibrium, the rate of formation of CD is equal to the the rate of decomposition of CD.
Therefore, the true statement is that after reaching equilibrium, the rate of forming products and reactants is the same.
In conclusion, a reaction at equilibrium has the forward and backward reactions occurring at the sane rate.
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A solution has a pOH of 7. 1 at 10∘c. Then the pH of the solution given that kw=2. 93×10−15 at this temperature is 7.4 .
It is given that,
pOH of solution = 7.1
Kw =2.93×10^(-15)
Firstly, we will calculate the value of pKw
The expression which we used to calculate the pKw is,
pKw=-log [Kw]
Now by putting the value of Kw in this expression,
pKw =−log{2.93×10^(-15)}
pKw =15log(2.93)
pKw=14.5
Now we have to calculate the pH of the solution.
As we know that,
pH+pOH=pKw
Now put all the given values in this formula,
pH+7.1=14.5
pH=7.4
Therefore, we find the value of pH of the solution is, 7.4.
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