Respuesta :
A solution containing 572.0ml of 0.6300mhcl is diluted to a volume of 1.000l. the ph of this solution is 0.4432
What is the ph of the given solution?
When the solution has been diluted to a volume of 1.000L, measure the concentration of H3O+ to determine the pH. Next, think about how HCl reacts with water.
HCl(aq)+H2O(l)⟶Cl−(aq)+H3O+(aq)
It is evident that there is exactly the same number of moles of HCl and H3O+ in the solution since the reaction continues to completion. A 0.6300M solution of 572.0 mL made up the initial solution.
Consequently, the following is what a mole of HCl is equal to:
nHCl=(572.0mLHCl)(1.000L/1,000mL)(0.6300MHCl)=0.3604molHCl
The 1:1 mole ratio enables us to see that:
(0.3604molHCl)(1molH3O+/1molHCl)
=0.3604molH3O+
Thus, the H3O+ concentration is as follows:
[H3O+]=0.3604mol/1.000L
=0.3604M
Therefore, the following formula is used to determine the solution's pH:
pH=−log(0.3604)=0.4432
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