If Kb for NX3 is 4.5×10−6, what is the pOH of a 0....

Question

If Kb for NX3 is 4.5×10−6, what is the pOH of a 0.175 M aqueous solution of NX3?Express your answer numerically.

Jules Bruno · Accepted Answer

We are being asked to calculate the pOH of a 0.175 M aqueous solution of NX3. NX3 has a low Kb, therefore we know that it is a weak base.Since we’re dealing with a weak base and Kb is an equilibrium expression, we will have to create an ICE chart to determine the equilibrium concentration of each species:• NX3 → weak base → proton acceptor• H2O → will act as the weak acid → proton donorEquilibrium reaction:       NX3(aq) + H2O(l) ⇌ NX3H+(aq) + OH-(aq)[readmore]Kb=productsreactantsKb=NX3H+OH-NX3Solids and liquids are not included in the expressionKb=xx0.175-xKb=x20.175-xNow, we need to determine if we can remove (–x) from the equation. To do so, we need to determine the ratio of the initial concentration and Kb: [NX3]initialKb=0.175 M4.5×10-6=38888>500Since the ratio is greater than 500, we can remove (–x) from the equation. The equation simplifies to:4.5×10-6=x20.175(0.175) 4.5×10-6=x20.175(0.175)7.875×10-7=x2x = 8.87412x10-4x = [OH-][OH-] = 8.87412x10-4 MCalculate the pOH of the solution from OH-:pOH=-log [OH-]pOH=-log [8.87412×10-4 M]pOH = 3.05The 0.175 M aqueous solution of NX3 solution has a pOH of 3.05.

Problem: If Kb for NX3 is 4.5×10−6, what is the pOH of a 0.175 M aqueous solution of NX3?Express your answer numerically.

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Problem Details

Problem: If Kb for NX3 is 4.5×10−6, what is the pOH of a 0.175 M aqueous solution of NX3?Express your answer numerically.

FREE Expert Solution

Problem Details

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