Calculate the amount of water you need to add (in mL) to 30mL of 1.5M HCl to dilute it to a concentration of 1.25M.
1.5M=1.5mol/dm3 And 0.30ml=30cm3=0.03dm3 So First We Find The No# Of Moles Of HCl Present n=M(conc)*vol(dm3)=1.5*0.03=0.045mol Using Mole Ratios NaOH+ HCl~>H2O+Nacl 1/1=0.045mol/x x=0.045mol Of H2O Therefore volume of a water n(0.045*1.25/1.5)/conc(1.25) now finish it by carying out the calculations
To answer this question, we can use the dilution formula:
C₁V₁ = C₂V₂
where:
C₁ is the initial concentration of the solution (1.5M HCl),
V₁ is the initial volume of the solution (30 mL of 1.5M HCl),
C₂ is the final concentration (1.25M),
and V₂ is the final volume of the diluted solution.
We need to find V₂, which represents the final volume of the diluted solution. Rearranging the formula gives us:
V₂ = (C₁V₁) / C₂
Substituting the given values, we get:
V₂ = (1.5M * 30 mL) / 1.25M
V₂ = 36 mL
Therefore, you need to add 36 mL of water to 30 mL of 1.5M HCl to dilute it to a concentration of 1.25M.