Question
In: Chemistry
50.0 mL of 1.00 M of a solution of HCl at 18.0 ºC is combined with...
50.0 mL of 1.00 M of a solution of HCl at 18.0 ºC is
combined with 50.0 mL of 1.00 M solution of NaOH at 18.0 ºC. The
final temperature of the reaction mixture is 24.6 ºC. If the heat
capacities and densities of these solutions are approximately the
same as water (4.184 J/g · ºC, 1.00 g/mL), what is the molar heat
of neutralization (∆Hneut.)? Is this reaction endothermic or
exothermic? [2 pt.]
HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l)
Solutions
Expert Solution
No of mole of HCl = 50*1/1000 = 0.05 mole
No of mole of NaOH = 50*1/1000 = 0.05 mole
total mass of mixture = d*V
= (50+50)*1 = 100 g
heat released in the reaction(q) = m*s*DT
= 100*4.184*(24.6-18)
= 2.7614 kj
enthalpy of neutralisation(DH0neu) = 2.7614 kj/0.05 mole
= 55.23 kj/mol
as temperature increases, it is exothermic process
queen_honey_blossom answered 2 years agoRelated Solutions
2.70g of Zn (s) reacts with 50.0 mL of 1.00 M HCl solution to produce hydrogen...
2.70g of Zn (s) reacts with 50.0 mL of 1.00 M HCl solution to
produce hydrogen gas according to the reaction. (R = 0.08206
L·atm·K-1·mol-
1)
Zn(s) + 2HCl (aq) = ZnCl2 (aq) + H2(g)
a) calculate mole of Zn used in this reaction
b) calculate mole of HCl used in this reaction
c) calculate which reactant is a limiting reactant
d) calculate mole of hydrogen gas formed
e) calculate volume of H2 gas at STP in Liters that will...
A student added 50.0 mL of an NaOH solution to 100.0 mL of 0.300 M HCl....
A student added 50.0 mL of an NaOH solution to 100.0 mL of 0.300
M HCl. The solution was then treated with an excess of aqueous
chromium(III) nitrate, resulting in formation of 2.36 g of
precipitate. Determine the concentration of the solution.
25.0 mL of a 4.21 M HCl solution at 25.2°C and 50.0 mL of a 2.50...
25.0 mL of a 4.21 M HCl solution at 25.2°C and 50.0 mL of a 2.50
M NaOH solution at 25.2°C are reacted together to give a final
temperature of 44.1°C. The specific heat of the solution is 3.88
J/g°C and it weighs 76.6 grams. From this information,
determine:
a. the limiting reactant for this reaction
b. the heat produced by the reaction (q) in units of Joules.
c. the enthalpy of the reaction (∆H) in units of kJ/mole.
When 18.0 mL of a 2.33×10-4 M aluminum acetate solution is combined with 22.0 mL of...
When 18.0 mL of a
2.33×10-4 M aluminum
acetate solution is combined with 22.0 mL
of a 4.80×10-4 M potassium
phosphate solution does a precipitate form? _____(yes or
no)
For these conditions the Reaction Quotient, Q, is equal to
_____?
When 18.0 mL of a 2.33×10-4 M aluminum acetate solution is combined with 22.0 mL of...
When 18.0 mL of a
2.33×10-4 M aluminum
acetate solution is combined with 22.0 mL
of a 4.80×10-4 M potassium
phosphate solution does a precipitate form? _____(yes or
no)
For these conditions the Reaction Quotient, Q, is equal to
_____?
a. When 18.0 mL of a 8.06×10-4 M aluminum chloride solution is combined with 15.0 mL...
a. When 18.0 mL of a
8.06×10-4 M aluminum
chloride solution is combined with 15.0
mL of a 5.62×10-4 M potassium
phosphate solution does a precipitate
form? (yes or no)
For these conditions the Reaction Quotient, Q, is equal to
b. When 25.0 mL of a
8.11×10-4 M iron(III)
nitrate solution is combined with 25.0 mL
of a 2.02×10-4 M sodium
sulfide solution does a precipitate form? (yes
or no)
For these conditions the Reaction Quotient, Q, is equal to .
c....
Consider a mixture of 50.0 mL of 0.100 M HCl and 50.0 mL of 0.100 M...
Consider a mixture of 50.0 mL of 0.100 M HCl and 50.0 mL of
0.100 M acetic acid. Acetic acid has a Ka of 1.8 x 10-5.
a. Calculate the pH of both solutions before mixing.
b. Construct an ICE table representative of this mixture.
c. Determine the approximate pH of the solution.
d. Determine the percent ionization of the acetic acid in this
mixture
A 100.0 ml sample of 1.00 M NaOH is mixed with 50.0 ml of 1.00 M...
A 100.0 ml sample of 1.00 M NaOH is mixed with 50.0 ml
of 1.00 M H2SO4 in a large Styrofoam coffee cup; the cup is fitted
with a lid through which passes a calibrated thermometer. the
temperature of each solution before mixing is 22.9°C. After adding
the NaOH solution to the coffee cup and stirring the mixed
solutions with thermometer; that the specific heat of the mixed
solutions is 4.18 J/(g•°C), and that no heat is lost to the...
A 50.0 mL solution of 0.167 M KOH is titrated with 0.334 M HCl . Calculate...
A 50.0 mL solution of 0.167 M KOH is titrated with 0.334 M HCl .
Calculate the pH of the solution after the addition of each of the
given amounts of HCl .
0.00 mL pH = 7.00 mL pH = 12.5 mL pH = 19.0 mL pH = 24.0 mL pH = 25.0 mL pH = 26.0 mL pH = 31.0 mL pH =
A 50.0 mL solution of 0.199 M KOH is titrated with 0.398 M HCl. Calculate the...
A 50.0 mL solution of 0.199 M KOH is titrated with 0.398 M HCl.
Calculate the pH of the solution after the addition of the
following amounts of HCl.
a) 0.00 mL HCl
b) 7.00 mL HCl
c) 12.5 mL HCl
d) 20.0 mL HCl
ADVERTISEMENT
ADVERTISEMENT
Latest Questions
- For Questions 1-3: consider the following code: public class A { private int number; protected String...
- You are tasked with assessing the health department’s intervention program in preventing recurrence of acute alcohol...
- Compare the MOSFET, JFET , and BJT and identify the reasons these devices behave differently. What...
- How would you use SAS Enterprise Miner to create a neural network model of your example?
- Explain the use of neural networking modeling in predictive analytics.
- Current Market Mix of Netflix, as detail as possible, please.
- This is all one question, thank you so much in advance! You must evaluate a proposal...
ADVERTISEMENT