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1 c.c. of 0.1N HCl is added to 99 CC solution of NaCl. The pH of the resulting solution will be
- a)7
- b)3
- c)4
- d)1
Correct answer is option 'B'. Can you explain this answer?
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1 c.c. of 0.1N HCl is added to 99 CC solution of NaCl. The pH of the r...
Volume of resulting solution = 100 ml
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1 c.c. of 0.1N HCl is added to 99 CC solution of NaCl. The pH of the r...
Given:
- Volume of 0.1N HCl = 1 cc
- Volume of NaCl solution = 99 cc
To find:
The pH of the resulting solution
Solution:
Step 1: Calculate the moles of HCl
- Concentration of HCl = 0.1 N
- Volume of HCl = 1 cc
Moles of HCl = Concentration × Volume
= 0.1 N × 1 cc
= 0.1 moles
Step 2: Calculate the moles of NaCl
- Concentration of NaCl = 0.1 N
- Volume of NaCl = 99 cc
Moles of NaCl = Concentration × Volume
= 0.1 N × 99 cc
= 9.9 moles
Step 3: Calculate the moles of H+ ions
- HCl dissociates in water to give H+ and Cl- ions
- The moles of H+ ions will be equal to the moles of HCl added
Moles of H+ ions = Moles of HCl
= 0.1 moles
Step 4: Calculate the total volume of the resulting solution
- The total volume of the resulting solution will be the sum of the volumes of HCl and NaCl solution
Total volume = Volume of HCl + Volume of NaCl solution
= 1 cc + 99 cc
= 100 cc
Step 5: Calculate the concentration of H+ ions
- Concentration is defined as moles of solute divided by the volume of the solution
Concentration of H+ ions = Moles of H+ ions / Total volume
= 0.1 moles / 100 cc
= 0.001 moles/cc
Step 6: Calculate the pH of the resulting solution
- pH is defined as the negative logarithm of the concentration of H+ ions
pH = -log10(Concentration of H+ ions)
= -log10(0.001 moles/cc)
= -(-3)
= 3
Answer:
The pH of the resulting solution will be 3.
- Volume of 0.1N HCl = 1 cc
- Volume of NaCl solution = 99 cc
To find:
The pH of the resulting solution
Solution:
Step 1: Calculate the moles of HCl
- Concentration of HCl = 0.1 N
- Volume of HCl = 1 cc
Moles of HCl = Concentration × Volume
= 0.1 N × 1 cc
= 0.1 moles
Step 2: Calculate the moles of NaCl
- Concentration of NaCl = 0.1 N
- Volume of NaCl = 99 cc
Moles of NaCl = Concentration × Volume
= 0.1 N × 99 cc
= 9.9 moles
Step 3: Calculate the moles of H+ ions
- HCl dissociates in water to give H+ and Cl- ions
- The moles of H+ ions will be equal to the moles of HCl added
Moles of H+ ions = Moles of HCl
= 0.1 moles
Step 4: Calculate the total volume of the resulting solution
- The total volume of the resulting solution will be the sum of the volumes of HCl and NaCl solution
Total volume = Volume of HCl + Volume of NaCl solution
= 1 cc + 99 cc
= 100 cc
Step 5: Calculate the concentration of H+ ions
- Concentration is defined as moles of solute divided by the volume of the solution
Concentration of H+ ions = Moles of H+ ions / Total volume
= 0.1 moles / 100 cc
= 0.001 moles/cc
Step 6: Calculate the pH of the resulting solution
- pH is defined as the negative logarithm of the concentration of H+ ions
pH = -log10(Concentration of H+ ions)
= -log10(0.001 moles/cc)
= -(-3)
= 3
Answer:
The pH of the resulting solution will be 3.
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1 c.c. of 0.1N HCl is added to 99 CC solution of NaCl. The pH of the resulting solution will bea)7b)3c)4d)1Correct answer is option 'B'. Can you explain this answer?
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