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Irina-Kira [14]
3 years ago
7

In step 6, khp was dissolved in a trivial amount of deionized h2o prior to titration with naoh. why was it acceptable to use an

approximate volume of h2o when this solution was used to determine the exact amount of naoh that was neutralized?
Chemistry
1 answer:
nadya68 [22]3 years ago
6 0
Water acts as solvent and it has no effect on the amount of the acid or the titrating agent. 
<span>Also, the concentration of the titrating agent must be known exactly, the amount of solvent is less important (the more diluted it is, the more accurate is the titration).</span>
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Answer:  Volume =  0.01L

Explanation:

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In this question, Mass = 1000g, Volume = ? and Density = 100 Kg/L

For the units to be uniform, we convert 1000g to Kg = 1Kg

Therefore, Volume = Mass / Density =  1Kg / 100Kg/L = 0.01L

                     

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For a process Arightwards harpoon over leftwards harpoonB, at 25 °C there is 10% of A at equilibrium while at 75 °C, there is 80
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This question is describing the following chemical reaction at equilibrium:

A\rightleftharpoons B

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Hence, we solve for the enthalpy change as follows:

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Learn more:

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