posted by tessa

This is the second reaction:
HCl(aq)+NaOH(aq)-->NaCl(aq)+H2O(l)
(Heat of neutralization)

This reaction involves mixing two solutions: 1.00 mol/L NaOH and 1.00 mol/L HCl.

Trial 1: 48.0 mL of the NaOH solution is mixed with 47.5 mL of the HCl. The temperature rises from 22.00°C to 27.90°C.

HINT:
Remember that you are heating water. Use the formula Q = C x M x DT. The volume of water used equals the volume of whatever solution you are using, be it NaOH or HCl. The volume must be converted to mass (1 mL of water has a mass of 1 g). The mass must be reported in kilograms.
In the second reaction you are using a solution of NaOH. To calculate the number of moles you must use the equation c= n/V. Also the final mass of water is the sum of the volumes of the NaOH solution and the HCl solution.

Questions:
1) Calculate the heat involved in the trial(Q)
2) Calculate the moles of NaOH used in the trial(mol)
3)Calculate how much heat would be evolved if 1 mole of NaOH was used (Q/mol)

1. DrBob222

Just follow the instructions given in questions 1, 2, and 3 along with the hint which tells you what to do.
Post your work if you have trouble.

2. tessa

I don't understand. in the formula Q=C*M*deltaT, do you use 4.200 kj/mol as C. Is the answer to question one, calculate the heat involved in the trial, 1.19 KJ?

3. DrBob222

The heat capacity of water is 4.18 J/g*K which is 4.18 kJ/kg*K (which I assume is why the question asks for mass in kg.
You have 48.0 mL + 47.5 mL = 95.5 mL and since the density of water is 1 g/mL, the solution has a mass of 95.5 g or 0.0955 kg.

## Similar Questions

1. ### chemistry

Could you help me get a definition for each of these words. for i can have a better understanding of them Thanx Titration gas collection crystalization fractional distillation solvent limiting reagent I have defined titration, gas …
2. ### Chemistry

I posted before about designing a procedure to determine two unknowns (1 solid, 1 solution). The possible solutions were: NaCl, CaCl2, CuSO4, NaOH,Ba(OH)2, HCl, HNO3, or H2O. The reagents given are: NaOH, HCl, AgNO3, Zn metal, Na2SO4, …
3. ### Chemistry

Which of these is true about the following reaction?
4. ### CHEM

Which of the following mixtures will result in the formation of a buffer solution when dissolved in 1.00 L of water?
5. ### Chemistry

Naoh (aq) + HCl (aq) --> NaCl (aq) + H2O (l) Using the dT determined in part 1, calculate the heat capacity of the calorimeter. Enthalpy of reaction= -58.3 kj/mol, Cs (NaCl = 3.91j/g C)density of 1 M NaCl = 1.037g/mL. dT= 12.88 …
6. ### chemistry

530 mL solution 10% HCl has been spilt onto the bench. It cannot be diluted or washed away. How much of the granular NaOH from the container seen in a must be used to neutralise the acid?
7. ### chemistry

50.0 mL of a solution of HCl is combined with 100.0 mL of 1.15 M NaOH in a calorimeter. The reaction mixture is initially at 22.4°C and the final temperature after reaction is 31.2°C. What is the molarity of the HCl solution?
8. ### Chemistry

Neutralization reaction HCL(aq) + NaOH(aq) -> NaCl(s) + H2O(l) Use your results to determine the netball change of the neutralization reaction, in kJ/mol of NaOH, Write the thermochemical equation for the neutralization reaction. …
9. ### chemistry

In a coffee cup calorimeter, 50 mL of 0.1 M HCl and 50 mL of 0.1 M NaOH are mixed to yield the following reaction: HCl + NaOH  NaCl + H2O. The two solutions were initially at 22.1 oC and the final temperature is 24.2 oC. Calculate …
10. ### Chemistry

Problem: Assume 200.0 mL of 0.400M HCl is mixed with 200.0 mL of 0.400M NaOH in a coffee-cup calorimeter. The temperature of the solutions before mixing was 25.10°C; after mixing and allowing the reaction to occur, the temperature …

More Similar Questions