A student mixes 40. Ml of 0. 10mhbr(aq) with 60. Ml of 0. 10mkoh(aq) at 25°c. What is the [oh−] of the resulting solution?
1 answer:
After the complete neutralization reaction occurs, excess hydroxide ion is left unreacted the hydroxide ion of the resulting solution, [OH-] is 0.02 M.
<h3>What is the concentration of the hydroxide ion, [OH-]?</h3>The hydroxide ion concentration is the amount in moles of hydroxide ion in a solution.
The hydroxide ion concentration is written as [OH-].
The equation of the reaction is given below:
1 mole of HBr reacts with 1 mole of KOH
Moles of HBr = 40 mL × 0.1 M = 4 mm moles
Moles of KOH = 60 mL × 0.1 M = 6 m moles
Moles of [OH-] = 6 - 4 = 2 m moles
Volume of solution = 100 mL
Thus, the concentration of the hydroxide ion, [OH-] is 0.02 M.
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The initial concentration of solution is 0.0693 M. The volume of solution taken is 10 mL and it is diluted to a final volume of 500 mL.
According to dilution law, the product of initial concentration and volume is equal to the product of final concentration and volume as follows:
Here, is initial concentration,
is final concentration,
is initial volume and
is final volume.
Rearranging to calculate final concentration,
Putting the values,
Therefore, concentration of the resulting solution is 0.001386 M.
Answer: The greatest concentration of C would be produced if the equilibrium constant of the reaction is equal to
Explanation:
Equilibrium constant is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric ratios. It is expressed as
For the given chemical reaction:
The expression for is written as:
Thus higher is the value of , higher will be the concentration of C. Thus the greatest concentration of C would be produced if the equilibrium constant of the reaction is equal to