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31 Cards in this Set
- Front
- Back
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chemical substance that can DONATE H+ or accept OH |
Acid |
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chemical substance that can ACCEPT H+ or donate OH |
Base |
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Acids and Bases react to form what |
Salts |
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activity = pH= |
Concentration -log [H+] |
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pOH +pH= |
14 |
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fully dissociate in solution |
Strong acids and strong bases |
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do not fully ionize (dissociate) in water, so [H+] is always < N |
Weak acids and weak bases |
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N x % ionizationn = |
[H+] or [OH-] |
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Concentration =
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amount of solute ----------------------- amount of solvent |
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Molartity = |
#moles ----------- volume |
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Normality = |
equivalents/volume (concentration) Molarity (M) x Valence |
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Calculate the [H+] of a solution with a pH of 12.6 |
12.6= - log [H+] 10^-12.6= H H= 2.51x10^-13 |
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Neutralization of an acid by a base involves what |
adding an equal amount of the opposing ion to form a salt N1V1 x N2V2 |
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What formula should you use when mixing two solutions |
N1V1 - N2V2 = NfVf |
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If NV (base) is > NV (acid ) you have excess _____ If NV (acid) is > NV (base) you have excess _____ |
[OH] [H] |
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What is the Henderson-Hasselbach equation |
pH = pKa + log [A]/[HA] [A]= conjugate base [HA}= acid |
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pKa > 7 = pKa < 7= |
weak base weak acid |
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Acids dissolve better in ____ solutions while base dissolve better in _____ solutions |
acid= basic solutions base= acidic solutions |
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is a mixture of a weak acid and its salt which resists change in pH when other acids or bases are added |
Buffer system |
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when 2 substances that ionize to form the same (common) ion are mixed in solution, the amount of dissociation is less than that expected if each were is solution on its own |
Common ion effect |
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_____ resist changesin pH and "absorb" excess acid an base |
Buffer |
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Calculate the pH of a buffer made from .15 M sodium acetate and .06 M acetic acid (pKa 4.76) |
pH= pKa + log [salt]/[acid] pH= 4.76 + log [.15]/[.06] pH= 5.16 |
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What are the known buffers and which is most important |
Bicarb (is most important) Phosphate Proteins |
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What formula should be used in calculating pCO2 |
pH= 6.1 + log [HCO3]/[H2CO3] |
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What does Ka represent |
its when 1/2 pKa is ionized; an equilibrium constant |
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Does a strong acid like HCL have a pKa |
No it fully dissociates |
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What makes up a buffer system |
weak acid/base salt |
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What is the mos timportant physiological buffer system |
Bicarb |
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What is the ratio o HCO3 to H2CO3 in blood at pH 7.4 |
20:1 |
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How do we measure te carbonic acid portion of the bicarbonate buffer system |
pCO2 |
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Are bases more solublein a basic solution or an acidic solution |
acidic |
