When solutions of silver nitrate and potassium chloride are mixed, silver chlori

Question

When solutions of silver nitrate and potassium chloride are mixed, silver chloride precipitates out of solution according to the equation AgNO3 (aq)-KCl(aq)AgCl(s)-KNO3 (aq) Part A What mass of silver chloride can be produced from 1.88 L of a 0.160 Msolution of silver nitrate? Express your answer with the appropriate units. Hints mass of AgCl = Submit 43.1 g My Answers Give Up Correct Part B The reaction described in Part A required 3.79 L of potassium chloride. What is the concentration of this potassium chloride solution? Express your answer with the appropriate units. Hints ] ? 0.0397M Submit My Answers Give Up Incorrect; Try Again; 5 attempts remaining

Explanation / Answer

AgNO3(aq)+ KCl (aq) -------->AgCl (s)+ KNO3(aq)

1 mole of AgNO3 reacts with 1 mole of KCl to give 1 mole of AgCl and 1 mole of KNO3.

moles of AgNO3= molarity* Volume in L= 0.160*1.88 =0.3008

molar mass of AgNO3= 170 g/mole, mass of AgNO3= moles* molar mass =0.3008*170 gm =51.14 gm

moles of KCl required= moles of AgNO3= 0.3008

concentration of KCl = moles/volume in L =0.3008/3.79= 0.079367 M

3 .mass of glucose = 20 gm, mass of glucose/100ml=20 g/100ml

=0.2 g/ ml, 1 ml of water contains 0.2 gm of glucose

45 ml of water contains 45*0.2=0.9 gm of glucose.

this is the amount that is present in 0.5L= 0.5*1000ml= 500ml

500ml of solution contains 0.9 gm of glucose

100ml of solution contains 100*0.9/500 =0.18 gm

Related Questions

Navigate

• Browse (All)
• Browse W
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.