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anonymous

  • 4 years ago

is the hydrogen ion concentration of a pH 3.8 solution higher or lower than that of a solution with a pH of 6.2?

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  1. anonymous
    • 4 years ago
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    wait explaing that a bit more if you dont mind

  2. Rogue
    • 4 years ago
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    pH = - log(based 10) [H+] [H+] = 10^(-pH)

  3. Rogue
    • 4 years ago
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    Use the second to find your hydrogen ion concentrations, you'll observe that the one with the lower pH has more hydrogen ions.

  4. Rogue
    • 4 years ago
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    For the solution with a pH of 3.8, [H+] = 10^-3.8 = 1.58 x 10^-4 M For the solution with a pH of 6.2, [H+] = 10^-6.2 = 6.31 x 10^-7 M The solution with a pH of 3.8 has a higher hydrogen ion concentration.

  5. anonymous
    • 4 years ago
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    how about if one solution has 100 times as many hydrogen ions as another solution, what is the difference, in pH units between the two solutions?

  6. Rogue
    • 4 years ago
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    10 to the what power gives you 100? :P

  7. anonymous
    • 4 years ago
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    2 :P

  8. Rogue
    • 4 years ago
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    So heres another question if you wanna try it: If the pH of a solution is 8.5, what is the pH of a solution that has a 10000 times greater hydrogen concentration?

  9. anonymous
    • 4 years ago
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    ok you got me but is the second question i asked you would that be 2 or negative 2?

  10. Rogue
    • 4 years ago
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    It would be 2.

  11. anonymous
    • 4 years ago
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    how so?

  12. anonymous
    • 4 years ago
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    or how would i show work sorry if im being annoying i jus dont understand this topic

  13. Rogue
    • 4 years ago
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    Its not your fault, I'm not really showing any work/explaining, sorry. Lets assume that solution A has a [H+] concentration greater than solution B. \[[H _{}^{+}]_{A}^{} = 10^{-pH _{A}^{}}\] \[[H _{}^{+}]_{B}^{} = 10^{-pH _{B}^{}}\]

  14. Rogue
    • 4 years ago
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    If we divide the two equations, we get that \[[H _{}^{+}]_{A}^{} / [H _{}^{+}]_{B}^{} =10^{-pH _{A}^{} + pH _{B}^{}} = 100\]

  15. anonymous
    • 4 years ago
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    ok i can see that

  16. Rogue
    • 4 years ago
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    \[10^{-pH _{A}^{} + pH _{B}^{}} = 100\] Take the log based 10 of both sides:\[\log_{10}( 10^{-pH _{A}^{} + pH _{B}^{}} = 100)\] \[{-pH _{A}^{} + pH _{B}^{}} = 2\]

  17. anonymous
    • 4 years ago
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    oh i see it now thanks! i am getting it a little now but if you dont mind i have about two other problems that need to be completed, but i dont exactly want you to do it for me but help me lead myself to an answer if you dont mind?

  18. Rogue
    • 4 years ago
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    Sure, I'll help :)

  19. anonymous
    • 4 years ago
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    alright thanks!!!!

  20. anonymous
    • 4 years ago
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    if solution a contains 1 x 10^-6 MH+ ions and solution B contains 1 x 10^-8 MH+ ions, which solution contains more H+ ions

  21. Rogue
    • 4 years ago
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    This question is just about your understanding of negative exponents I guess. Convert the numbers from scientific notation to standard notation to see which one is bigger.

  22. anonymous
    • 4 years ago
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    ok dang i feel dumb now lol but do you know the relationship between hydrogen ion contrecations to the acidity and alklinity (basicity) of solution?

  23. Rogue
    • 4 years ago
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    An easier way to do this problem would be to look at the pH's of each solution. If you look at the [H+] equation and compare it to the values they give, you'll notice that the first solution has a pH of 6 whilst the second has a pH of 8.

  24. anonymous
    • 4 years ago
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    so would the ph of 6 be greater right?

  25. Rogue
    • 4 years ago
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    Higher hydrogen ion concentration = lower pH = more acidity. Lower hydrogen ion concentration = higher pH = more basicity.

  26. Rogue
    • 4 years ago
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    Yup, the pH of 6 has more...

  27. anonymous
    • 4 years ago
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    awesome!!!!!!!!!!!

  28. Rogue
    • 4 years ago
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    You'll get the hang of these problems after a while. Remember the key concepts and those two equations.

  29. anonymous
    • 4 years ago
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    HA is an acid that ionizes 10% in a solution. what is the H+ of a 0.01 M solution of HA? what is its pH?

  30. anonymous
    • 4 years ago
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    would the ph be 1 or 2?

  31. anonymous
    • 4 years ago
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    oh and thanks again for all the help

  32. Rogue
    • 4 years ago
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    If 10% of the 0.01 M is ionized, how much H+ are there?

  33. anonymous
    • 4 years ago
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    um yeah now ya got me

  34. anonymous
    • 4 years ago
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    -2?

  35. Rogue
    • 4 years ago
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    10% of 0.01 M is just 0.001 M, so that is you H+ concentration. pH = - log [H+] = - log (0.001) = 3

  36. Rogue
    • 4 years ago
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    pH is often positive by the way, unless your dealing with a strong acid, or a super concentrated solution.

  37. anonymous
    • 4 years ago
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    so would 3 be the pH or the HA? or the amount of H+?

  38. Rogue
    • 4 years ago
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    pH = 3, H+ = 0.001 M

  39. Rogue
    • 4 years ago
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    HA is just some arbitrary acid, H is for the hydrogen an acid has, and A is for acid.

  40. anonymous
    • 4 years ago
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    when did you lean all this stuff?

  41. anonymous
    • 4 years ago
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    or where?!

  42. Rogue
    • 4 years ago
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    Last year, took ap chem :)

  43. anonymous
    • 4 years ago
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    like a boss!!!!

  44. anonymous
    • 4 years ago
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    alright so in this next problem it seems like its working backwards what is the H+ of a solution whose pH is 8? what is the OH-?

  45. Rogue
    • 4 years ago
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    Use these equations to help you: pH + pOH = 14 pH = - log [H+] pOH = - log [OH-] [H+] = 10^-pH [OH- ] = 10^-pOH

  46. Rogue
    • 4 years ago
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    So for the first part, [H+] = 10^-8 M. For the second part, you get pOH = 6, so then [OH-] = 10^-6 M

  47. Rogue
    • 4 years ago
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    I've got an ap bio final tomorrow, so I gotta go to sleep. Try to solve your problems using the equations I gave you, good luck! :D

  48. anonymous
    • 4 years ago
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    alright good luck on your final and thanks!

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