# 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

Dear Student,

1)  0.1 M HCl acid

pH = - loge [H+]
so as the concentration is 0.1 M = 10-1
So, pH = - loge [10-1]
pH = 1

Similarly, 2) 0.1 M H2SOacid
pH = - loge [H+]
so as the concentration is 0.1 M = 10-1
So, pH = - loge​​​​​​​ [10-1]
pH = 1

3) 0.05 M HNO3 acid​​​​​​​
pH = - loge [H+]
so as the concentration is 0.05 M = 5 × 10-2
So, pH = - loge​​​​​​​ [5 × 10-2]
ph = - { log 5 - 2 log10 }
pH = - { 0.69 - 2}
= 1.31

4) 0.05 M H3PO4
pH = - loge [H+]
so as the concentration is 0.05 M = 5 × 10-2
So, pH = - loge​​​​​​​ [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 (H2SO4) and hydrochloric acid (HCl) are strong acids (both dissociate readily in aqueous solution).

At the same molarity (moles per liter), H2SO4 has twice the number of available hydronium ions as HCl. So H2SO4 would be roughly twice as acidic, and therefore be a stronger acid. Similar with the case of H3PO4, therefore it is stronger acid at same molarity.

Hope this information will clear your doubts about the topic.

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Regards

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