At Westonci.ca, we make it easy for you to get the answers you need from a community of knowledgeable individuals. Connect with a community of experts ready to help you find accurate solutions to your questions quickly and efficiently. Discover in-depth answers to your questions from a wide network of professionals on our user-friendly Q&A platform.
Sagot :
Answer:
[tex]pH\text{ = }2.75[/tex]Explanation:
Here, we want to get the pH of the given molecule
Firstly,we write the ionization equation so as to get the number of hydrogen atoms from its dissociation
We have this as:
[tex]HCOOH_{(aq)}+H_2O_{(l)}\rightleftarrows HCOO^-_{(aq)}+H_3O^+_{(aq)}[/tex]The Pka value for formic acid is 3.75
We have it that:
[tex]\begin{gathered} K_a=10^{-pKa} \\ K_a=10^{-3.75}\text{ = }1.78\text{ }\times10^{-4} \end{gathered}[/tex]Using the ICE equation for the equilibrium constant,we have it that:
[tex]K_a\text{ = }\frac{\lbrack HCOO^-\rbrack\lbrack H_3O^+\rbrack}{\lbrack HCOOH\rbrack\rbrack}[/tex]Thus, we have:
[tex]0.000178=\frac{x^2}{0.018\text{ - x}}^{}[/tex]Since x is very small as opposed to tthe initial acid concentration, we approximate x as 0 below
Thus,we have:
[tex]\begin{gathered} (0.018\times0.000178)=x^2 \\ x\text{ = }\sqrt[]{0.018\times0.000178} \\ x\text{ = 0.00179} \end{gathered}[/tex]Finally, we know that the pH is the negative logarithm to base 10 of the concentration of hydroxonium ion
[tex]\begin{gathered} pH=-log\lbrack H_3O^+\rbrack_{} \\ pH\text{ = -log\lbrack{}0.00179\rbrack} \\ pH\text{ = 2.75} \end{gathered}[/tex]
We appreciate your time. Please come back anytime for the latest information and answers to your questions. Thank you for your visit. We're dedicated to helping you find the information you need, whenever you need it. Thank you for using Westonci.ca. Come back for more in-depth answers to all your queries.
