pH

• Acids have more H+ than OH-, while bases have more OH- than H+
• A solution with a pH of 7 has an equal number of H+ and OH- ions
• pH = a measure of how acidic or basic a chemical is when it's in an aqueous (water) solution.
• neutral pH value = 7
• pH level > 7 = basic / bases
• pH level < 7 = acidic / acid
• Increasing hydrogen ion [H+] concentration decreases pH
• Decreasing hydroxide ion [OH-] concentration increases pH
• ACIDIC = Most fruits, vegetables, and body fluids
• If there's no water, there's no pH

  •  no pH value
  • vegetable oil
  • gasoline
  • pure alcohol
• Danish biochemist Søren Peter Lauritz Sørensen = equation of calculating pH

  • pH = -log[H+]
• pH 5 = Human skin, hair, and nails
• pH 7.0 = pure water
• simplest method = pH paper test strips
• most accurate method = pH meter
• "pH" comes from the German word "potenz" + H (hydrogen) = Power of Hydrogen
• human blood has a pH level of 7.4
• BUFFER SOLUTION = maintains a balance in the pH to avoid shift in the pH level
• BUFFER SOLUTION = made up of weak acid & conjugate base or weak base & conjugate acid ; to maintain pH balance by resisting strong acids/bases added to the solution
• BUFFER PREPARATION = solution made from weak acid and adding conjugate base or combining weak base with conjugate acid.
• a strong acid, like hydrochloric acid (HCl) is added to lower the pH of acidic buffers
• A strong base, like sodium hydroxide solution (NaOH), is added to increase the pH of alkaline buffers.
• BUFFER CAPACITY = the amount of a strong acid or base that a buffer solution can take before significant pH changes occur
• The smaller the value of Ka, the stronger the acidity
• The larger the value of Ka, the weaker the acidity
• any change in the human blood larger than 0.10 pH unit = ILLNESS
• if pH of human blood goes below 6.8 or above 7.8 = DEATH
• to maintain pH level of 7.4 in the human body = BUFFER SYSTEMS: CABONATES, PHOSPHATES, PROTEINS
• most important buffer system = CARBONATE BUFFER (carbonic acid - bicarbonate ion)

  • 10:1 ratio
  • body increase or decrease depending on the number of acids entering the blood
  • most metabolic wastes = ACIDS (lactic acid ) & KETONES
• second most important buffer system = PHOSPHATE (sodium dihydrogen phosphate - sodium hydrogen phosphate ion)

  • 1:6 ratio = 1 ratio to maintain 7.4
• almost ALL PROTEINS = buffers

  • proteins made up of amino acids (+amino grp & -carboxyl grp)
  • buffering by proteins = 2/3 of buffering power of the blood and most of the buffering within cells.
• normal arterial blood pH = narrow range of 7.35 to 7.45

  • slight change = pathologic conditions (metabolic or respiratory)
• 6 - 7.35 = ACIDOSIS

  7.35 - 7.45 = NORMAL

  7.45 - 9 = ALKALOSIS

  
• ACIDOSIS = overproduction of acid in the body fluids or the blood

  • pH falls below 7.35
  • caused by excessive loss of bicarbonate or build up of carbon dioxide = poor lung function or depressed breathing
• ALKALOSIS = excessive blood alkalinity in the body fluids or the blood

  • pH rises above 7.45 and above 7.8 is deadly
  • caused by loss of acid or low level of carbon dioxide = rapid / deep breathing, cognitive impairment, numbness in the extremities, muscle spams, vomiting