1. Why isn't the mass of potassium sulfate used in any of the calculations? 2. If the barium sulfate precipitate is not dried thoroughly, will the experimentally determined concentration be higher or lower than the true value? Concisely explain based on how the molarity is calculated. 3. An experimenter reacts 30.0 mL of a BaCl, solution with excess AgNO, as shown in the unbalanced equation below. If 2.58 grams of AgCl are obtained, what is the molarity of BaCl solution? Hint: First balance the chemical equation. 2.S8 2AGNO3(aq) BaCl2 (aq) QAGCI(s) Ba(NO3)2(aq) a.se Imol 1243,5 I 07. 00 T

Question

Question 3

1. Why isn't the mass of potassium sulfate used in any of the calculations?
2. If the barium sulfate precipitate is not dried thoroughly, will the experimentally determined
concentration be higher or lower than the true value? Concisely explain based on how the molarity
is calculated.
3. An experimenter reacts 30.0 mL of a BaCl, solution with excess AgNO, as shown in the
unbalanced equation below. If 2.58 grams of AgCl are obtained, what is the molarity of BaCl
solution?
Hint: First balance the chemical equation.
2.S8
2AGNO3(aq)
BaCl2 (aq)
QAGCI(s)
Ba(NO3)2(aq)
a.se
Imol
1243,5
I
07.
00
T
Expand
Transcribed Image Text

1. Why isn't the mass of potassium sulfate used in any of the calculations? 2. If the barium sulfate precipitate is not dried thoroughly, will the experimentally determined concentration be higher or lower than the true value? Concisely explain based on how the molarity is calculated. 3. An experimenter reacts 30.0 mL of a BaCl, solution with excess AgNO, as shown in the unbalanced equation below. If 2.58 grams of AgCl are obtained, what is the molarity of BaCl solution? Hint: First balance the chemical equation. 2.S8 2AGNO3(aq) BaCl2 (aq) QAGCI(s) Ba(NO3)2(aq) a.se Imol 1243,5 I 07. 00 T

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