Problem: A solution is prepared by adding 50.0 mL of 0.050 M HBr to 150.0 mL of 0.10 M HI. Calculate [H+] and the pH of this solution. HBr and HI are both considered strong acids.

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FREE Expert Solution

pH=-log[H+]


Molarity(M)=moles of soluteLiters of solution


  • HBr → H+ + Br-
    • moles HBr = moles H+
  • HI → H+ + I-
    • moles HI = moles H+


[H+]=total moles H+total volume of solution[H+]=50.0 mL×10-3 L 1 mL×0.050 mol H+L  sol'n+150.0 mL×10-3 L 1 mL×0.10 mol H+L sol'n(50.0 + 150.0 ) mL×10-3 L1 mL[H+]=0.0175 mol H+0.20 L sol'n

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Problem Details

A solution is prepared by adding 50.0 mL of 0.050 M HBr to 150.0 mL of 0.10 M HI. Calculate [H+] and the pH of this solution. HBr and HI are both considered strong acids.

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Our tutors have indicated that to solve this problem you will need to apply the Strong Acid-Base Calculations concept. If you need more Strong Acid-Base Calculations practice, you can also practice Strong Acid-Base Calculations practice problems.

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Based on our data, we think this problem is relevant for Professor Oliver's class at UCSC.

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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl 2nd Edition practice problems.