What is the molar mass of NaCl?

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Molar mass refers to the mass of 1 mole of a substance. The molar mass of NaCl (sodium chloride), also called table salt, is 58.44 g/mol.

Step 1 – To calculate it, the atomic masses of sodium (Na) and chlorine (Cl) and their respective amounts in the chemical formula of NaCl are needed.

The atomic mass of sodium is 22.99 g/mol and the atomic mass of chlorine is 35.45 g/mol.

Step 2 – Molar Mass Formula = Atomic mass of element x no. of atoms in subscript

Step 3 – In NaCl, there is one sodium ion (Na⁺) and one chloride ion (Cl^-), so the molar mass of NaCl can be calculated as:

Molar Mass of NaCl = Mass of Na + Mass of Cl

= (1 x 22.99 g/mol) + (1 x 35.45 g/mol)

= 22.99 g/mol + 35.45 g/mol

= 58.44 g/mol

So, the molar mass of NaCl is 58.44 g/mol.

NaCl Molar Mass

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Mole Fraction	Moles to Grams	Difference between Molar Mass and Molecular Mass
Molarity Formula	Relation Between Molarity and Molality	Molecular Formula
Concentration of a Solution	Abnormal Molar Masses	Molecular Weight Formula

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What is the molar mass of NaCl?

CBSE CLASS XII Related Questions

1.
Explain: (i) Presence of carbonyl group in glucose. (ii) Presence of five $-$OH groups attached to different carbon atoms.

2.
Give structures of A, B and C: $CH_3Cl \xrightarrow{KCN}$ A $\xrightarrow{LiAlH_4}$ B $\xrightarrow{CHCl_3 + \text{alc. } KOH, \Delta}$ C

3.
Why is o-nitrophenol more acidic than o-methoxyphenol?

4.
61 g benzoic acid (M = 122 g mol$^{-1}$) dissolved in 500 g benzene. Vapour pressure of pure benzene = 66 torr. Assume complete dimerisation. Calculate vapour pressure of solution.

5.
Under what condition can a bimolecular reaction become kinetically first order?

6.
For decomposition of $H_2O_2$ by $I^-$: Step I: $H_2O_2 + I^- \rightarrow H_2O + IO^-$ (slow). Step II: $H_2O_2 + IO^- \rightarrow H_2O + I^- + O_2$ (fast). (a) Write rate law. (b) Determine order w.r.t. $H_2O_2$ and $I^-$ and overall order. (c) Molecularity of Step II.

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What is the molar mass of NaCl?

CBSE CLASS XII Related Questions

1.Explain: (i) Presence of carbonyl group in glucose. (ii) Presence of five $-$OH groups attached to different carbon atoms.

2.Give structures of A, B and C: $CH_3Cl \xrightarrow{KCN}$ A $\xrightarrow{LiAlH_4}$ B $\xrightarrow{CHCl_3 + \text{alc. } KOH, \Delta}$ C

3.Why is o-nitrophenol more acidic than o-methoxyphenol?

4.61 g benzoic acid (M = 122 g mol$^{-1}$) dissolved in 500 g benzene. Vapour pressure of pure benzene = 66 torr. Assume complete dimerisation. Calculate vapour pressure of solution.

5.Under what condition can a bimolecular reaction become kinetically first order?

6.For decomposition of $H_2O_2$ by $I^-$: Step I: $H_2O_2 + I^- \rightarrow H_2O + IO^-$ (slow). Step II: $H_2O_2 + IO^- \rightarrow H_2O + I^- + O_2$ (fast). (a) Write rate law. (b) Determine order w.r.t. $H_2O_2$ and $I^-$ and overall order. (c) Molecularity of Step II.

Comments

SUBSCRIBE TO OUR NEWS LETTER

1.
Explain: (i) Presence of carbonyl group in glucose. (ii) Presence of five $-$OH groups attached to different carbon atoms.

2.
Give structures of A, B and C: $CH_3Cl \xrightarrow{KCN}$ A $\xrightarrow{LiAlH_4}$ B $\xrightarrow{CHCl_3 + \text{alc. } KOH, \Delta}$ C

3.
Why is o-nitrophenol more acidic than o-methoxyphenol?

4.
61 g benzoic acid (M = 122 g mol$^{-1}$) dissolved in 500 g benzene. Vapour pressure of pure benzene = 66 torr. Assume complete dimerisation. Calculate vapour pressure of solution.

5.
Under what condition can a bimolecular reaction become kinetically first order?

6.
For decomposition of $H_2O_2$ by $I^-$: Step I: $H_2O_2 + I^- \rightarrow H_2O + IO^-$ (slow). Step II: $H_2O_2 + IO^- \rightarrow H_2O + I^- + O_2$ (fast). (a) Write rate law. (b) Determine order w.r.t. $H_2O_2$ and $I^-$ and overall order. (c) Molecularity of Step II.