Concentration terms such as mass percentage,$ppm$,mole fraction,and molality are independent of temperature,whereas molarity is a function of temperature. Explain.
(N/A) Molarity of a solution is defined as the number of moles of solute dissolved in $1 \ L$ of solution. Since volume depends on temperature and changes with it,molarity also changes with temperature.
On the other hand,concentration terms like mass percentage,$ppm$,mole fraction,and molality are based on mass-by-mass relationships.
Since mass does not change with temperature,these concentration terms remain independent of temperature variations.
On the other hand,concentration terms like mass percentage,$ppm$,mole fraction,and molality are based on mass-by-mass relationships.
Since mass does not change with temperature,these concentration terms remain independent of temperature variations.
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Similar Questions
Which of the following statements is true?
$(1)$ $200 \ mL$ of $0.2 \ M \ NaOH$ has the same number of moles of solute as $1000 \ mL$ of $1 \ M \ NaOH$.
$(2)$ $200 \ mL$ of $1 \ M \ NaOH$ has the same number of moles as $1000 \ mL$ of $0.2 \ M \ NaOH$.
$(3)$ $100 \ mL$ of $0.2 \ M \ NaOH$ has the same number of moles as $1000 \ mL$ of $1 \ M \ NaOH$.
$(4)$ $2000 \ mL$ of $0.2 \ M \ NaOH$ has the same number of moles as $1000 \ mL$ of $1 \ M \ NaOH$.
$(1)$ $200 \ mL$ of $0.2 \ M \ NaOH$ has the same number of moles of solute as $1000 \ mL$ of $1 \ M \ NaOH$.
$(2)$ $200 \ mL$ of $1 \ M \ NaOH$ has the same number of moles as $1000 \ mL$ of $0.2 \ M \ NaOH$.
$(3)$ $100 \ mL$ of $0.2 \ M \ NaOH$ has the same number of moles as $1000 \ mL$ of $1 \ M \ NaOH$.
$(4)$ $2000 \ mL$ of $0.2 \ M \ NaOH$ has the same number of moles as $1000 \ mL$ of $1 \ M \ NaOH$.
What mass of ethanol in $g$ must be added to $1.0 \, kg$ of water to have a mole fraction of ethanol equal to $0.2$?
Medium
View SolutionIn $500 \ mL$ of $0.2 \ M \ NaCl$ solution,$1500 \ mL$ of $0.4 \ M \ MgCl_2$ solution is mixed. The only incorrect final concentration of ion is (assume volume to be additive)
In an aqueous glucose solution,the mole fraction of water is $40$ times the mole fraction of glucose. What is the weight percentage $(w/w)$ of glucose in the solution?
The mole fraction of the solute in a $1 \ m$ (molal) aqueous solution is:
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