HCL is tritrated with NaOH. KHP is then added. A possible source of systematic error in this experiment is failure to dry the KHP. If this occured, would the final wt% NA2CO3 be falsely high, falsely low, or unaffected. Give reasoning. Thanks.

You have left out much of the problem. I can't believe KHP is added after titrating HCl with NaOH. And where does the Na2CO3 come in? I know but you might be able to determine the answer yourself if you organized the facts of the experiment a little better. Please reread and repost with a cleaner post.

It is not certain what you are doing. How is sodium carbonate entering the reaction.

Normally, one uses KHP to determine the molarity of NaOH. If the KHP were wet, too little mass for KHP (some of what you massed was water) would have been recorded, so the molarity of the sodium hydroxide would have been calculated as too low. How this error of low molarity of NaOH affects the rest of the experiment depends on what you did.

Based on the information provided, it seems that there may be some confusion or missing details in the experiment description. However, I can still provide some general information regarding the potential effect of failure to dry the KHP on the final weight percent of Na2CO3.

KHP (potassium hydrogen phthalate) is commonly used as a primary standard for acid-base titrations as it can be accurately weighed and has a known stoichiometry. NaOH (sodium hydroxide) is often used as the titrant to determine the concentration of an acid solution.

Assuming that the Na2CO3 mentioned in the question is not relevant to the experiment, and solely focusing on the titration of HCl with NaOH followed by KHP addition, failure to dry the KHP could introduce a systematic error in the experiment.

If the KHP is not dried, it may contain residual moisture. The moisture will add to the measured mass of the KHP, resulting in an overestimation of the amount of KHP used. As a result, the calculated concentration of NaOH will be lower than the actual value.

If the concentration of NaOH is lower than it should be, it will affect the subsequent calculations involving the weight percent of Na2CO3, assuming it is part of the experiment. The calculated weight percent of Na2CO3 could be falsely low because the concentration of NaOH, which is used in the calculations, is underestimated.

In summary, failure to dry the KHP can lead to an overestimation of its mass and subsequently result in an underestimation of the concentration of NaOH. This can potentially lead to a falsely low weight percent of Na2CO3, assuming it is relevant to the experiment.

Please provide more specific details or clarify the experiment setup if further assistance is required.