Example #3) 15mL of 2.0M HCI is mixed with 30mL of 0.75M KOHHCI + KOH → H₂O + KCIAHreaction =SubstanceH₂OHC1KC1KOHAHreaction=AHproducts-AHreactantsAHreaction = (AHH20+ AHKCI) - (AHHCI + AHKOH)AHreaction = (-286+ -419- 1kg1Let's calculate the limiting reagent to determine how many mols of water will be formed:Remember: Volume of reactant ÷ 1000 x Molarity of reactant x mole-to-mole ratio to waterHere's the first reactant: 15mL of 2.0M HCIIS1500* 2.00.03 mol HCl301000Lof LOM KOHLet's do this for the second reactant, 30mL of 0.75M KOH0.750.0225 mol KOH=-)-(-164-61mol H₂O) xAHf in kJ/mol-286-164-419-480The limiting reagent is the compound that produced the fewest number of moles. Multiply thatnumber of moles buy the AH reaction that was calculated abovekJ/mol = -/-3725 kJ-+_ - 48010.0225CalcuFrom here on out, you are on your own! Calculate the enthalpy of reaction, and then thelimiting reagent. Next multiply the enthalpy of reaction by the limiting reagent. Good luck! Example #4) 50mL of 1.5M HCI is mixed with 60mL of 1.0M KOHHCI + KOH → H₂O + KCIAHf in kJ/mol-286-164-419-480Note: this is the same reaction as example #3, so the AH reaction should be the sameSubstanceH₂OHCIKCIKOHAHreaction=AHproducts- AHreactantsAHreaction =-bikiLet's calculate the limiting reagent to determine how many mols of water will be formed:Here's the first reactant: 50mL of 1.5M HCI50 * 1.5.10001.5 = 0.075 mol HelLet's do this for the second reactant, 60mL of 1.0M KOH601000* 1 = 0.obmolkottCalculate the amount of energy released:Call 0.06 * -61 = -3.66 kg

Dear student Since you have posted multiple questions, we will solve only first question for you if…

Answered: Example #3) 15mL of 2.0M HCl is mixed…

Science

Chemistry

Example #3) 15mL of 2.0M HCl is mixed with 30mL of 0.75M KOH

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: A 15.0 mL solution of Sr(OH)2 is neutralized with 42.7 mL of 0.350 M HCI. What is the concentration…

A: The reaction involved is Sr (OH)2 + 2 HCl → SrCl2 + 2 H2O

Q: Calculate the pH at the equivalence point when 75.0 mL of 0.250 M HCl is mixed with 0.350 M of…

Q: If 5.0ml of a 1.0m HCL solution is required to consume all the Na2CO3 in 15.0 mL of a solution what…

Q: Using 12.16 m hcl and 3 m naoh calculate how to make 100 ml of 0.1 M of each

A: Given that,Initial concentration of HCl (M1) = 12.16 MFinal concentration of HCl (M2) = 0.1 MFinal…

Q: How many grams of KHCOO (MM = 84.12 g/mol) must be added to 1.00 L of 0 838 M HCOOH to make a buffer…

A: A buffer solution is an aqueous solution. It consist of a mixture of a weak acid and its conjugate…

Q: Which of the following species would be more soluble in 0.100 M HCl than in pure water (CIRCLE ALL…

A: NaF : it acts a strong electrolyte and dissociates to form F- ions which form strong hydrogen…

Q: When 25.0 mL of 0.650 M NaOH is titrated with HCl, 37.19 mL are required to reach the endpoint. What…

Q: Question 10 Which of the following statements about buffered solu- tions are true? Select all that…

A: Buffer solution: A buffer solutions is an aqueous solution consisting of a mixture of a weak base…

Q: What is the pH if I mix 20.0 mL of 0.100 M HAc, 30.00 of .100 M NaOH, and 20.0 mL of distilled H2O?

A: pH is the measure of acidity or basicity of a solution. Mathematically, it is the negative…

Q: use the following set of data to answer the questions below; 20.00 ML of 0.100 M NaOH was titrated…

A: Given, 20.00 ML of 0.100 M NaOH was titrated with 16.71 ml of 0.0600 M H2SO4

Q: If [NaOH]= 0.0930M and it was determined that it took 18.5mL of NaOH to reach the equivalence point…

A: Given,

Q: Which of the following mixtures are capable of tolerating addition of a strong base without altering…

Q: 0.4201 g of a unknown monoprotic acid was dissolved in 25.00 mL of water and titrated with 0.09995 M…

Q: When the CaSO4 is 2.4 x 10^-5 what would be the volume of H2O to dissolve .33g of CaSO4

A: The maximum amount of solute that can dissolve in a known quantity of solvent at a certain…

Q: Why do we have to standardize the NaOH solution before we can determine the %v/v concentration of…

A: Vinegar is a watery acetic solution that can contain flavorings with trace chemicals. The average…

Q: 2) The indicator Haln has Ka = 4.5 x 105, Kaz = 4.5 x 10°. H,ln is red, HIn' is blue, In2 is yellow.…

A: Given data:-

Q: What is pOH of a solution consisting of 1.35 M NH3 and 2.08 M NH&NO;? K, of NH, is 5.8 x 10 t0 0 494…

A: The pH of the solution is related with the pOH of the solution by the following relation, pH + pOH =…

Q: I titrate a sample of aqueous sulfuric acid with 14.27mL and 0.117M Potassium hydroxide. Calculate…

Q: What percent of a 0.0138 M NaCN solution undergoes hydrolysis? [K, for HCN-3.98E-10] 0.182 4.27…

A: Answer:-This question is answered by using the simple concept of calculation of degree of hydrolysis…

Q: How many moles of HCI are there in 75.0 mL of 0.170 M HCI?

Q: A 20.0 mL solution of NaOH is neutralized with 26.3 mL of 0.200 M HBr. What is the concentration of…

Question

Example #3) 15mL of 2.0M HCI is mixed with 30mL of 0.75M KOH
HCI + KOH → H₂O + KCI
AHreaction =
Substance
H₂O
HC1
KC1
KOH
AHreaction=AHproducts-
AHreactants
AHreaction = (AHH20+ AHKCI) - (AHHCI + AHKOH)
AHreaction = (-286
+ -419
- 1kg1
Let's calculate the limiting reagent to determine how many mols of water will be formed:
Remember: Volume of reactant ÷ 1000 x Molarity of reactant x mole-to-mole ratio to water
Here's the first reactant: 15mL of 2.0M HCI
IS
1500
* 2.0
0.03 mol HCl
30
1000
Lof LOM KOH
Let's do this for the second reactant, 30mL of 0.75M KOH
0.75
0.0225 mol KOH
=
-)-(-164
-61
mol H₂O) x
AHf in kJ/mol
-286
-164
-419
-480
The limiting reagent is the compound that produced the fewest number of moles. Multiply that
number of moles buy the AH reaction that was calculated above
kJ/mol = -/-3725 kJ
-
+_ - 480
10.0225
Calcu
From here on out, you are on your own! Calculate the enthalpy of reaction, and then the
limiting reagent. Next multiply the enthalpy of reaction by the limiting reagent. Good luck!

Example #4) 50mL of 1.5M HCI is mixed with 60mL of 1.0M KOH
HCI + KOH → H₂O + KCI
AHf in kJ/mol
-286
-164
-419
-480
Note: this is the same reaction as example #3, so the AH reaction should be the same
Substance
H₂O
HCI
KCI
KOH
AHreaction=AHproducts- AHreactants
AHreaction =
-biki
Let's calculate the limiting reagent to determine how many mols of water will be formed:
Here's the first reactant: 50mL of 1.5M HCI
50 * 1.5.
1000
1.5 = 0.075 mol Hel
Let's do this for the second reactant, 60mL of 1.0M KOH
60
1000
* 1 = 0.obmolkott
Calculate the amount of energy released:
Call 0.06 * -61 = -3.66 kg

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps with 1 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

21
Indicate whether compound A and B is soluble or insoluble
If a 0.552M HCl caq) solution is used by a scientist to titrate 10.00mL of a weak base, based curve (shown below), what base? write your the titration the concentration of the auswer with 4 decitual places. pH Curve OM is 12 10 8 6 4 2 0 5:0 2 1.5 n 3 3.5 A Volume of Titrant / mL 7.5 8 8.5
How do I tell which salt is more soluble in certain instances? (ex: 1.0M H+ versus pure water)
None
Which of the following graphs describes the relationship between the pH of a buffer and the volume of NaOH added to the buffer? А. В. pH pH Volume of NaOH added Volume of NaOH added С. D. pH pH Volume of Volume of NAOH added NAOH added
Assume that: • Acid 1 is a stronger acid that Acid 2. You prepare two separate solutions, using 1.0 mol of each acid and mixing it with 1.0 L of pure water. Determine which of the following statements is correct. Select all that apply. O Multiple answers: Multiple answers are accepted for this question Select one or more answers and submit. For keyboard navigation... SHOW MORE V a Acid 1 has a larger K value that Acid 2. b Acid 1 will generate a higher concentration of H,0* ions. The solution prepared using Acid 1 will have a lower pH. d. Acid 1 will generate a higher concentration of A- ions. e The concentration of unreacted "HA" at equilibrium for the Acid 1 solution will be lower. f The pK value for Acid 1 is lower than the pK value for Acid 2.
Construct a graph and plot the titration curve for a 10.0 mL aliquot of 0.100 mol/L NH3 (pKb=4.74) with 0.100 mol/L HCl. For this purpose, make a table with nine added volumes of HCl solution, which you consider adequate, with the corresponding pH value. Write the development of all calculations and use approximate formulas.
2. How many of the following pairs could be used to create a buffer if mixed in a 1:1 mole ratio? (select all that apply, wrong choices will be penalized) KOH and HNO3 HCl and NaCl H2CO3 and KHCO3 HCl and NaOH HF and NaF NH4Cl and NH3 HNO2 and NaNO2 HCl and NH3 HC2H3O3 and KC2H3O3