PLEASE SHOW WORK/EXPLAIN Please show work.... 1. A 10.00 mL choride sample requi

Question

PLEASE SHOW WORK/EXPLAIN Please show work.... 1. A 10.00 mL choride sample required 33.65 mL of .01251 M AgNO3 to reach the end point. a) How many moles of Cl- were present in the sample? b) What was the molarity of the Cl- sample? 2. Would the following errors increase, decrease, or not change the molarity of Cl- as calculated in part 1b? Explain your answer (use a calculation if needed). a) The student was past the end point of the titration when the final volume was recorded. b) The student incorrectly read the molarity of AgNO3 as 0.01521 M

Explanation / Answer

1) solutions for a& b

Cl-   + AgNO3 ------------------> AgCl + NO3-

moles of AgNO3 completely react with moles of Cl- because it is 1:1 reaction

so 10.00 x C = 33.65 x 0.1251

C = 0.421 M

molarity of Cl- sample = 0.421 M

moles of Cl- = molarity x volume

                     = 0.421 x 10 / 1000

                    = 4.21 x 10^-3

moles of Cl- = 4.21 x 10^-3

2)

a)

molarity of Cl- decreased. because volume is lesser amount measured so moles of AgNO3 also lesser and moles of Cl- decreases molarity decreases

b)

in this case increases , if molarity of AgNO3 more and we get Cl- molarity also more we get , because the relation is

M1 V1 = M2 V2

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