Please help me answer these. Can you include the work as best you can as well? Thanks! Even if you can only answer one, that would be so so so much help, seeing as im totally lost!
1. What mass of KBr would be needed to prepare 500mL of 1.5M solution?
2. If 750.0 ML of an AgNO3 reacts with enough copper to produce 0.52g of Ag by single displacement, What is the molarity of AgNO3? given equation: 2AgNO3+Cu --> 2Ag+Cu(NO3)2
3.When ammonia dissolves in water, it reaches the equilibrium describe by this equation NH3(aq)+H2O(L) <--> NH4^+(aq)+OH^-(aq). The value of the equilibrium constant is 1.8x10^-5. If [NH3}=0.25M and [NH4]=0.075M, what is the concentration of OH^-?
4.write the product solubility constant for MgBr2-
Write the equilibrium constant expression, forward reaction, and reverse reaction for the following-
5. AgCl(s) <=> Ag^+(aq) + Cl^- (aq)
6. H2(g)=Cl2(g) <=> 2HCl(g)
1. What mass of KBr would be needed to prepare 500mL of 1.5M solution?
2. If 750.0 ML of an AgNO3 reacts with enough copper to produce 0.52g of Ag by single displacement, What is the molarity of AgNO3? given equation: 2AgNO3+Cu --> 2Ag+Cu(NO3)2
3.When ammonia dissolves in water, it reaches the equilibrium describe by this equation NH3(aq)+H2O(L) <--> NH4^+(aq)+OH^-(aq). The value of the equilibrium constant is 1.8x10^-5. If [NH3}=0.25M and [NH4]=0.075M, what is the concentration of OH^-?
4.write the product solubility constant for MgBr2-
Write the equilibrium constant expression, forward reaction, and reverse reaction for the following-
5. AgCl(s) <=> Ag^+(aq) + Cl^- (aq)
6. H2(g)=Cl2(g) <=> 2HCl(g)
-
1. Atomic weights" K=39, Br = 80, KBr=119. Let the solution be called S.
500mLS x 1.5molKBr/1000mLS x 119gKBr/1molKBr = 89g KBr to two significant figures.
2. Atomic weight6: Ag=108. Let the AgNO3 solution be called S.
0.52gAg/750.0mLS x 1000mLS/1LS x 1molAg/108gAg x 1molAgNO3/1molAg = 0.0064 mole/L to two significant figures
3. If [NH4+} = 0.075, then [OH-] = 0.075 also
4. MgBr2 is very soluble in water. Therefore, the Ksp of MgBr2 is infinite.
5. ,K = [Ag+][Cl-}; K = 1/[Ag+][Cl-]
6. K = [HCl]^2/[H2][Cl2]; K = [H2][Cl2]/[HCl}^2
500mLS x 1.5molKBr/1000mLS x 119gKBr/1molKBr = 89g KBr to two significant figures.
2. Atomic weight6: Ag=108. Let the AgNO3 solution be called S.
0.52gAg/750.0mLS x 1000mLS/1LS x 1molAg/108gAg x 1molAgNO3/1molAg = 0.0064 mole/L to two significant figures
3. If [NH4+} = 0.075, then [OH-] = 0.075 also
4. MgBr2 is very soluble in water. Therefore, the Ksp of MgBr2 is infinite.
5. ,K = [Ag+][Cl-}; K = 1/[Ag+][Cl-]
6. K = [HCl]^2/[H2][Cl2]; K = [H2][Cl2]/[HCl}^2