What volume (in mL) of 3.75×10^−2 M HNO3 is needed to titrate 45.0 mL of 1.15×10^−2 M LiOH to the equivalence point?
Balanced chemical equation is:
LiOH + HNO3 ---> LiNO3 + H2O
Here:
M(LiOH)=0.0115 M
M(HNO3)=0.0375 M
V(LiOH)=45.0 mL
According to balanced reaction:
1*number of mol of LiOH =1*number of mol of HNO3
1*M(LiOH)*V(LiOH) =1*M(HNO3)*V(HNO3)
1*0.0115 M *45.0 mL = 1*0.0375M *V(HNO3)
V(HNO3) = 13.8 mL
Answer: 13.8 mL
What volume (in mL) of 3.75×10^−2 M HNO3 is needed to titrate 45.0 mL of 1.15×10^−2...
what volume of 5.00X10^-3 M HNO3 is needed to titrate 80.00 mL of 5.00X 10^-3 M Ca(OH)2 to the equivalence point
How many milliliters of 0.821 M HNO3 are needed to titrate each of the following solutions to the equivalence point? (a) 50.6 mL of 1.07 M NaOH mL (b) 40.0 mL of 0.657 M RbOH mL (c) 498.0 mL of a solution that contains 17.7 g of LiOH per liter mL
What volume of 0.114 M HCl is needed to titrate 25.0 mL of 0.172 M pyridine (C5H5N) to its equivalence point? For pyridine, pKb = 8.77.
Be sure to answer all parts. Find the pH and the volume (mL) of 0.487 M HNO3 needed to reach the equivalence point in the titration of 2.65 L of 0.0750 M pyridine (C5HzN, Kb = 1.7 x 10-9). Volume = mL HNO3 pH-
What volume (in mL) of 0.1899 M NaOH is required to titrate 15.00 mL of 0.1559 M HAc to the equivalence point? (give your answer to 2 decimal places)
Determine the volume in mL of 0.57 M HNO3(aq) needed to reach the half-equivalence (stoichiometric) point in the titration of 37.9 mL of 0.5 M CH3NH2(aq)(aq). The Kb of methylamine is 3.6 x 10-4. Enter your answer with two decimal places and no units. (how is the answer 16.62?)
How many mL of the titrant HBr is needed to titrate 8.41 mL of 0.044 M NH2CI, if the molarity of the titrant is 0.088? What is the pH of a solution that contains 0.50 M H3PO4 and 0.89 M NaH2PO4? The Ka of H3PO4 is 7.5x10-3. How many mL of the titrant HBr is needed to titrate 8.41 mL of 0.044 M NHCl, if the molarity of the titrant is 0.088? What is the pH of when 0.066 L...
titration:
2. If 45.0 mL of 1.50 M Ca(OH)2 are needed to neutralize 25.0 mL of HI of unknown concentration, what is the molarity of the HI? How many mL of 0.100 M NaOH are needed to titrate 20.0 mL of 0.100 M H2SO4?
What volume of 0.0850 M HCl is required to titrate 25.00 mL of a 0.100 M NH3 solution to the equivalence point?? Please show work so I can understand -- thank you.
17.42 How many milliliters of 0.105 M HCl are needed to titrate each of the following solutions to the equivalence point: (a) 45.0 mL of 0.0950 M NaOH, (b) 22.5 mL of 0.118 M NH3, (c) 125.0 mL of a solution that contains 1.35 g of NaOH per liter?