Chapter 11

Equations M = n/V M 1 V 1 = M 2 V 2 if the moles are the same n 1 n 2 you can cancel out the n’s. pH = -log [H + ] pOH = -log [OH - ] pH + pOH = 14 [H 3 O + ] = 10^ -pH [OH - ] = 10^ -pOH [H 3 O + ] [OH - ] = 1.0 x

1) KCl, CaBr 2, Al(NO 3 ) 3 a) How many moles of each ion are in an aqueous solution? Assume you start with one mole of each salt.

1) KCl, CaBr 2, Al(NO 3 ) 3 b) What is the molarity of each ion in 0.500L of water?

Ex. 2) If mL of 0.100M HCl and mL of 0.100M NaOH are mixed, what is the molarity of the salt in the resulting soln? (Assume the volumes are additive)

Ex. 3) If 100.0mL of 0.100M HCl and mL of M NaOH are mixed, what are the molarities of the solutes in the resulting soln? What is the pH? (HCl, NaOH, and NaCl are strong electrolytes)

Ex. 4) What volume of M HCl soln would neutralize 30.0 mL of M Ca(OH) 2

Ex. 5) Find the molarity of 37.7 mL of HCl when it is titrated with 42.2 mL of 0.236M NaOH. What is the pH of the acid?

Ex. 6) A mL sample of 0.275M lithium hydroxide completely reacts with mL of phosphoric acid. What is the molarity of the acidic solution?

Ex. 7) if [OH - ] = 7.2 x M what is the pH? Ex. 8) when pH = what is [H 3 O + ]?

Ex. 9) [H 3 O + ]= x M, pOH = ? Ex. 10) [HNO 3 ] = 2.4 M, what is the pH?

Ex. 11) [H 2 SO 4 ] = M, what is the pH? Ex. 12) pH = ? When [Sr(OH) 2 ] = 1.55 x M

Ex. 13) How many mL of concentrated 12 M HCl will you need to make L of M HCl? What is the initial pH? What is the resulting pH? Ex. 14) You add 500. mL of water to 500. mL of 1.25 M NaOH. What is the pH of the resulting solution?

 A g sample of an impure Iron(II) sulfate is titrated with mL of M potassium permangante to the endpoint. What is the % purity of the ferrous sulfate?