Question

In: Chemistry

What amount of water is formed when 20 mL of 0.80 M HCl and 30 mL...

What amount of water is formed when 20 mL of 0.80 M HCl and 30 mL of 0.40 M NaOH are mixed?

Solutions

Expert Solution

The balanced equation is

NaOH + HCl -----> NaCl + H2O

Number of moles of NaOH = molarity * volume of solution in L

Number of moles of NaOH = 0.40 * 0.030 L = 0.012 mole

Number of moles of HCl = 0.80 * 0.02 L = 0.016 mole

From the balanced equation we can say that

1 mole of NaOH requires 1 mole of HCl so

0.012 mole of NaOH will require

= 0.012 mole of NaOH *( 1 mole of HCl / 1 mole of NaOH)

= 0.012 mole of HCl

But we have 0.016 mole of HCl which is in excess so NaOH is limiting reactant

From the balanced equation we can say that

1 mole of NaOH produces 1 mole of H2O so

0.012 mole of NaOH will produce 0.012 mole of H2O

mass of 1 mole of H2O = 18.015 g so

the mass of 0.012 mole of H2O = 0.216 g

Therefore, the mass of H2O produced would be 0.216 g


Related Solutions

20 mL of 4.0 M acetone + 10 mL of 1.0 M HCl + 20 mL...
20 mL of 4.0 M acetone + 10 mL of 1.0 M HCl + 20 mL of 0.0050 M I2 If the reaction is zero order in I2, approximately how long would it take for the I2 color to disappear at the temperature of the reaction mixture 20 mL of 4.0M acetone + 10 mL of 1.0 M HCl + 10 mL 0f 0.0050M I2 + 10 mL H2O .
what is the pH of: water 50.0 mL water + 1.0 mL 1.0 M HCl 50.0...
what is the pH of: water 50.0 mL water + 1.0 mL 1.0 M HCl 50.0 mL water + 1.0 mL 1.0 M NaOH 0.10 M acetic acid 0.10 M sodium acetate
a) How many moles of water are formed when 28.0 mL of 0.250 M HNO3 and...
a) How many moles of water are formed when 28.0 mL of 0.250 M HNO3 and 53.0 mL of 0.320 M KOH are mixed? b) What is the concentration of H+(aq) and OH–(aq) after the reaction is complete?
Calculate the pH in the titration of 20 mL of 0.125 M HCL with 0.250 M...
Calculate the pH in the titration of 20 mL of 0.125 M HCL with 0.250 M NaOH solution after adding 9.60 mL and 10.40 mL of NaOH
When 50.0 mL of 0.45 M HCl was added to 50.0 mL of 0.65 M NaOH,...
When 50.0 mL of 0.45 M HCl was added to 50.0 mL of 0.65 M NaOH, the temperature change was 5.8 *C. Calculate the heat change for the reaction (Qsoln) and the heat of neutralization (ChangeHneut), and the state whether the reaction is exothermic or endothermic.
When 50.0 mL of 0.45 M HCl was added to 50.0 mL of 0.65 M NaOH,...
When 50.0 mL of 0.45 M HCl was added to 50.0 mL of 0.65 M NaOH, the temperature change was 5.8 *C. Calculate the heat change for the reaction (Qsoln) and the heat of neutralization (ChangeHneut), and the state whether the reaction is exothermic or endothermic.
If the density of water is 1g/mL and the density of a 0.16 M HCl solution...
If the density of water is 1g/mL and the density of a 0.16 M HCl solution is 1.023 g/mL, how do I use this information to determine the mass of both water and HCl in one liter of the solution? ***Cancel this question! I figured it out!
2. For the titration of 20 mL of 0.1026 M NH3 with 0.09747 M HCl, calculate...
2. For the titration of 20 mL of 0.1026 M NH3 with 0.09747 M HCl, calculate the pH before the addition of titrant, at 10 mL prior to the equivalence point, at the equivalence point, and at 10 mL after the equivalence point. Ka (NH4+) = 5.7 x 10-10
1. What is the change in pH when 10.0 mL of 0.010 M HCl is added...
1. What is the change in pH when 10.0 mL of 0.010 M HCl is added to 500 mL of pure water. 2. What is the change in pH when 10.0 mL of 0.010 M NaOH is added to 500 mL of pure water.
When 35.0 mL of 1.43 M NaOH at 22.0oC are neutralized by 35.0 mL of HCl...
When 35.0 mL of 1.43 M NaOH at 22.0oC are neutralized by 35.0 mL of HCl also at 22.0oC in a coffee cup calorimeter, the temperature of the final solution rises to 31.29oC. The specific heat of all solutions and the density of all solutions is the same as that of water. Calculate the heat of neutralization for one mole of HCl. Please show all work with the correct answer. Thank you!!!!
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT