4. How many milliliters of 0.0844 M Ba(OH)2 are required to titrate 50.00 mL of

Question

4. How many milliliters of 0.0844 M Ba(OH)2 are required to titrate 50.00 mL of 0.0526 M HNO:? 5. A 25.00 mL sample of 0.132 M nitric acid is mixed with 10.00 mL of 0.318 M potassium hydroxide. Is the resulting solution acidic, basic, or exactly neutralized? 6. Silver nitrate reacts with copper(I1) chloride. a) Write the molecular equation. b) Write the total ionic equation. c) Write the net ionic equation. 7. Hydrobromic acid reacts with calcium sulfite. a) Write the molecular equation. b) Write the total ionic equation. c) Write the net ionic equation

Explanation / Answer

Ans 4

Calculuate number of moles of HNO3 you are going to titrate:
Molarity X Volume = moles
(0.0526M) X (.050L) = .00263 moles of HNO3

Ba(OH)2 + 2HNO3 -> 2H2O + Ba(No3)2

we can see that 2 moles of HNO3   neutralizes one mole of Ba(OH)2 .

So, .00263 moles of HNO3 will neutralise (1/2)*0.00263 moles of Ba(OH)2

  0.00131 moles of Ba(OH)2

There are TWO OH- in Ba(OH)2 so concentration of OH- is two times concentration ofBa(OH)2 : 2( 0.0844M )= 0.169M

volume in liters = moles/Molarity

(.00131 moles)/(.169M) = 7.75X10^-3 L = 7.75mL

ans 5.

a) AgNO3  + CuCl2 -> AgCl2 + Cu(NO3)2

b) Net ionic equation
2Ag+(aq) + 2Cl-(aq) --> 2AgCl(s)
simplify:
Ag+(aq) + Cl-(aq) --> AgCl(s)

c)complete ionic equation:
2Ag+(aq) + 2NO3-(aq) + Cu2+(aq) + 2Cl-(aq) --> 2AgCl(s) + Cu2+(aq) + 2NO3-(aq)

ans

a) CaSO3(s)+2HBr(aq)CaBr2(aq)+SO2(g)+H2O(l)

b) total ionic equation

CaSO3(s) + 2H+(aq) + 2Br-(aq) Ca2+(aq) + 2Br-(aq) + SO2(g) + H2O(l)

c) ionic equation

CaSO3(s)+2H+(aq)Ca2+(aq)+SO2(g)+H2O(l)

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