Respuesta :
Answer : The calculated molarity of the NaOH solution would be lower than the actual .
Explanation :
In the standardization of NaOH using KHP, an accurately weighed sample of KHP is used. KHP is a primary standard which means it is highly stable and does not absorb water. Therefore it can be used to standardize reagents used for the chemical reaction.
The reaction of KHP with NaOH gives a salt KP- and water.
The net ionic equation for this reaction is written below.
[tex]KHP (aq)+ OH^{-} (aq)\rightarrow KP^{-}(aq)+ H_{2}O (l)[/tex]
The amount of NaOH consumed during the reaction depends upon the amount of KHP. If the sample is contaminated with NaCl, then some of the mass of KHP would be replaced by NaCl. As a result, we have less amount of KHP available to react with NaOH than the actual.
This would give us less amount of NaOH , because part of the KHP is replaced by NaCl which is non reactive .
This would result in lower molarity of NaOH solution.
The concentration of NaOH will be too high.
KHP stands for potassium hydrogen phthalate. It is often used as a primary standard because it can be obtained in pure form and it is not deliquescent so it can be accurately weighed and used as primary standard.
The net ionic equation of the process is; H^(aq) + OH^-(aq) ------> H2O(l). We can see that sodium ions are spectator ions in the reaction. The concentration of KHP is determined by weighing out the mass of the standard and dissolving in a known volume of water.
If the KHP is inadvertently contaminated with NaCl, the calculated concentration of NaOH will be too high because we will have a higher value for the concentration of KHP than accurate.
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