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How Much Acid is Too Much?
Target 7-2
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What We Know The pH of normal ocean water is_____
The pH of the oceans now is ________ Rivers keep the ocean pH stable by ____________
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What We Know The pH of normal ocean water is 8.1-8.2
The pH of the oceans now is ________ Rivers keep the ocean pH stable by ____________
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What We Know The pH of normal ocean water is 8.1-8.2
The pH of the oceans now is Rivers keep the ocean pH stable by ____________
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What We Know The pH of normal ocean water is 8.1-8.2
The pH of the oceans now is Rivers keep the ocean pH stable by acting as a buffer
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Recap Acids are substances that increase the amount of H3O+ in a sample
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Recap Weak Acids: Dissociate partially (not completely)
Stay at equilibrium Ex) C2H5COOH + H2O <-> C2H5COO- + H3O+
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Recap When a weak acid dissociates, it creates its conjugate base
Ex) C2H5COOH + H2O <-> C2H5COO- + H3O+
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Recap Conjugate Base: a molecule made when an acid loses its acidic hydrogen Acts like a very weak base Is able to react with H+ to re-form the original acid
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Buffers A buffer solution is a solution containing a weak acid and its conjugate base or a weak base/conj. acid Solution is at equilibrium Will react with a strong acid or strong base
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Buffers Remember that when acid is added to water, H3O+ ions are formed: HCl H+ + Cl- H+ + H2O H3O+
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Buffers When acid is added to a buffer solution, those H+ ions react with the weak base in the buffer before they react with the water HCl H+ + Cl- H+ + H2O + NaHCO3 NaH2CO3 + H2O The H3O+ ion doesn’t form, so the pH changes less
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Demo We are going to add strong acid to water and to a buffer solution. Record the pH of each solution after each drop is added.
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Reflect What happened when we added acid to water?
What happened when we added acid to the buffer?
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In the Ocean Primary Ocean Buffer System: Na2CO3 + H+ <-> NaHCO3
NaCO3 is formed when: Carbonate ions (CO32-) from bedrock flow from rivers into the ocean Carbonate reacts with sodium ions (Na+) from the salt in ocean water
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