Home
Class 11
CHEMISTRY
0.6 mmol of NaCI and 1 mol of HCI in 1 L...

`0.6` mmol of NaCI and 1 mol of `HCI` in 1 L solution is a buffer.

Text Solution

AI Generated Solution

To determine whether the statement "0.6 mmol of NaCl and 1 mol of HCl in 1 L solution is a buffer" is true or false, we need to analyze the components of the solution. ### Step-by-Step Solution: 1. **Identify the Components**: - We have **0.6 mmol of NaCl** (sodium chloride) and **1 mol of HCl** (hydrochloric acid) in a 1 L solution. 2. **Define a Buffer**: ...
Promotional Banner

Topper's Solved these Questions

  • IONIC EQUILIBRIUM

    CENGAGE CHEMISTRY ENGLISH|Exercise Archives Multiple Correct|3 Videos

  • IONIC EQUILIBRIUM

    CENGAGE CHEMISTRY ENGLISH|Exercise Archives Single Correct|25 Videos

  • IONIC EQUILIBRIUM

    CENGAGE CHEMISTRY ENGLISH|Exercise Exercises Integer|10 Videos

  • HYDROGEN, WATER AND HYDROGEN PEROXIDE

    CENGAGE CHEMISTRY ENGLISH|Exercise Subjective Archive (Subjective)|3 Videos

  • ISOMERISM

    CENGAGE CHEMISTRY ENGLISH|Exercise Assertion-Reasoning Type|1 Videos

Similar Questions

Explore conceptually related problems

The pH of a solution containing 0.1mol of CH_(3)COOH, 0.2 mol of CH_(3)COONa ,and 0.05 mol of NaOH in 1L. (pK_(a) of CH_(3)COOH = 4.74) is:

When 0.01 moles of NaOH are added to 1 litre of a buffer solution , its pH changes from 4.745 to 4.832. The buffer capacity is

What is the pH of the solution when 0.20 mol of HCI is added to 1L of a solution containing a. 1M each of acetic acid and acetate ion. b. 0.1M each of aceta acid and acetate ion. Assume the total volume is 1L. K_(a) for acetic acid is 1.8 xx 10^(-5) .

How much moles of sodium propionate should be added to 1L of an aqueous solution containing 0.020 mol of propionic acid to obtain a buffer solution of pH 4.75 ? What will be the pH if 0.010 mol of HCI is dissolved in the above buffer solution. Compare the last pH value with the pH of 0.010 M HCI solution. Dissociation constant of propionic acid, K_(a) , at 25^(@)C is 1.34 xx 10^(-5) .

The p^(H) of 0.1 M NaCI solution is

Calculate the minimum mass of NaCI necessary to dissolve 0.01mol AgC1 in 100L solution. (Assume no change in volume) (K_(f)AgC1_(2)^(Θ) = 2.5 xx 10^(5)) (K_(sp)AGCl = 2 xx 10^(-10))

Electrolysis of an 1 M HCI solution liberates

Whenever an acid is neutralised by a base, the net reaction is H^(o+)(aq)+overset(Theta)OH(aq)rarr H_(2)O(l),DeltaH =- 57.1 kJ Calculated the heat evolved for the following experiments? 0.50 mol of HCI solution is neutralised by 0.50mol of NaoH solution.

Buffer capacity of a buffer solution is x , the volume of 1 M NaOH added to 100 mL of this solution if the change of pH by 1 is

A buffer solution is made by mixing a weak acid HA (K_(a) =10^(-6)) with its salt NaA in equal amounts. What should be amount of acid or salt that should be added to make 90 mL of buffer solution in which if 0.1 mole of strong acid are added into 1 L of this buffer solution then change in pH is unity ?