How Much Sodium Bicitrate Is Required for a pH 5.42 Solution?

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To prepare a 1.00 L solution with a pH of 5.42, the concentration of hydronium ions [H3O+] is calculated as 10^-5.42. The discussion highlights confusion regarding sodium bicitrate and its role in the equilibrium expression for its dissociation. Participants express difficulty in determining the necessary mass of sodium bicitrate without understanding its chemical properties. Additionally, the relationship between pH and pOH is mentioned, indicating that pOH can be derived from the pH value. Clarifying these concepts is essential for solving the problem effectively.
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Homework Statement


What mass of sodium bicitrate would be needed to prepare a 1.00 L solution with a pH of 5.42?


Homework Equations


[H30+]=10^-pH


The Attempt at a Solution


First of all, I don't know what sodium bicitrate is, so I can't write the equation for it. What's bicitrate?

I wanted write the equilibrium expression for Ka. But I can only find the concentration of the [H30+] and not anything else... I have no idea how to do this question. Help please?
 
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if pH = 5.42, what is pOH equal to?

then [OH-] = 10^-pOH
 
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