# The acid solution with higher ph value is 1. 0.1 M HCl acid 2. 0.1 M H2SO4 acid 3. 0.05 M HNO3 acid 4. 0.05 M H3PO4 acid

1) 0.1 M HCl acid

pH = - log

_{e}[H

^{+}]

so as the concentration is 0.1 M = 10

^{-1}

So, pH = - log

_{e}[10

^{-1}]

pH = 1

Similarly, 2) 0.1 M H

_{2}SO

_{4 }acid

pH = - log

_{e}[H

^{+}]

so as the concentration is 0.1 M = 10

^{-1}

So, pH = - log

_{e} [10

^{-1}]

pH = 1

3) 0.05 M HNO

_{3}acid

pH = - log

_{e}[H

^{+}]

so as the concentration is 0.05 M = 5 × 10

^{-2}

So, pH = - log

_{e} [5 × 10

^{-2}]

ph = - { log 5 - 2 log10 }

pH = - { 0.69 - 2}

= 1.31

4) 0.05 M H

_{3}PO

_{4}

pH = - log

_{e}[H

^{+}]

so as the concentration is 0.05 M = 5 × 10

^{-2}

So, pH = - log

_{e} [5 × 10

^{-2}]

ph = - { log 5 - 2 log10 }

pH = - { 0.69 - 2}

= 1.31

Now,

The strength of an acid depends on the concentration of hydronium ions formed in solution. Both sulfuric acid (H_{2}SO_{4}) and hydrochloric acid (HCl) are strong acids (both dissociate readily in aqueous solution).

At the same molarity (moles per liter), H_{2}SO_{4} has twice the number of available hydronium ions as HCl. So H_{2}SO_{4} would be roughly twice as acidic, and therefore be a stronger acid. Similar with the case of H_{3}PO_{4}, therefore it is stronger acid at same molarity.

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