Molarity = mol/L
density= grams/ mL
this is a conversion problem where we have to change the numerator from grams to moles, and the denominator from ml to L.
First, we need our conversion factors
1 liters= 1000 mililters
to convert the mass to moles, we need the molar mass of the compound acetic acid (CH3<span>COOH)
molar mass of </span>CH3<span>COOH is </span><span>60.05 g/mol, which can be calculated by going to the periodic table and add the mass of the each atom in the compound formula.
1.049 g/ ml (1 mol/ 60.05 grams)= 0.0175 mol/ ml
0.0175 mol/ ml (1000 ml/ 1 liters)= 17.5 mol/ L or 17.5 M
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Answer:
There are <span>1.479×<span>10<span>−13</span></span></span> concentration of hydrogen ions <span>mo<span>lL</span></span>.
Explanation:
Because pH is a logarthmic scale, we can use the formula: <span><span>[<span>H+</span>]</span>=<span>10-pH</span></span>. Where...
=> <span>[<span>H+</span>]</span> is the concentration of hydrogen ions in the solution.
=> <span>pH</span> is the pH of the solution.
=> Where 10 is the base of the power - it's a logarithm formula.
We can now just sub in the values and solve for [<span><span>H+</span>]</span>.
<span><span><span>[<span>H+</span>]</span>=<span>10-pH</span></span><span><span>=<span>10<span>−<span>(12.83)</span></span></span></span><span>=1.479108388×<span>10<span>−13</span></span></span></span></span>
We can round (if required) to <span>1.479×<span>10<span>−13</span></span></span>.
Thus, there are <span>1.479×<span>10<span>−13</span></span></span> concentration of hydrogen ions <span><span>mol</span>L</span>.
Hope this helps :)
Without that cell it would die.