What is the pH of a 0.090 M #HCl# solution? Chemistry Acids and Bases Acids and Bases 1 Answer anor277 Aug 9, 2016 #pH=-log_10[H_3O^+]#, so......... Explanation: #HCl(aq) + H_2O(l) rarr H_3O^+ + Cl^-# And thus #pH=-log_10(0.090)# #=# #-(-1.05)# #=# #1.05#. What is #pOH# of this solution? Answer link Related questions How do resonance structures affect acidity? How does carbon dioxide change the acid-base condition of a solution? Why do strong acids have a low pH? Is neutralization a double replacement reaction? Why is NaH a strong base? Is HBr a strong acid? Is HF a strong acid? Why does neutralization occur? Do strong acids completely dissociate in water? How can I calculate pH of weak acid? See all questions in Acids and Bases Impact of this question 3764 views around the world You can reuse this answer Creative Commons License