1 / 17

Electrolysis 2NaCl(aq) + 2H 2 O(l)  → 2Na + (aq) + 2OH - (aq) + H 2 (g) + Cl 2 (g)

Electrolysis 2NaCl(aq) + 2H 2 O(l)  → 2Na + (aq) + 2OH - (aq) + H 2 (g) + Cl 2 (g). Define Electrolytes. Substances like acid, base and salts which can conduct electricity in their aqueous solution due to ionization are known as electrolytes. Strong Electrolytes.

seven
Download Presentation

Electrolysis 2NaCl(aq) + 2H 2 O(l)  → 2Na + (aq) + 2OH - (aq) + H 2 (g) + Cl 2 (g)

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Electrolysis2NaCl(aq) + 2H2O(l) →2Na+(aq) + 2OH-(aq) + H2(g) + Cl2(g)

  2. Define Electrolytes • Substances like acid, base and salts which can conduct electricity in their aqueous solution due to ionization are known as electrolytes

  3. Strong Electrolytes • Some electrolytes such as potassium chloride, sodium hydroxide, sodium nitrate are completely ionized in their constituent ions in solution. • These electrolytes are known as strong electrolytes. In other words strong electrolytes are 100% dissociated in their aqueous solution.

  4. Weak Electrolytes • Electrolytes which are weakly ionized in their aqueous solution are called as weak electrolytes. • In the aqueous solution of weak electrolytes, the constituent ions are in equilibrium with un-dissociated molecules of electrolytes. 

  5. List of strong electrolytes • Chloric acid • Nitric acid • Potassium hydroxide • Calcium hydroxide • Sodium chloride • Potassium nitrate

  6. List of Weak Electrolytes • Acetic acid • Ammonium hydroxide • Carbonic Acid • Nitrous Acid • Tap Water ( Pure Water is Non-Electrolytes)

  7. Electrolytes • Some chemical compounds play an important role for cells in the body to function and allow the body to work are called as electrolytes. • Electrolytes allow cells to generate energy and maintain the stability of their wall. • Electrolytes are present in the human body, and the balance of the electrolytes in our bodies is essential for normal function of our cells and our organs.

  8. Normal Adult Values  • Calcium: 4.5-5.5 mEq/L • Chloride: 97-107 mEq/L • Potassium: 3.5-5.3 mEq/L • Magnesium: 1.5-2.5 mEq/L • Sodium: 136-145 mEq/L • Phosphate :2.4 - 4.4 mg/dL.

  9. Sodium (Na+ ) • Sodium is the major positive ion (cation) in fluid outside of cells • Hypernatremia( too much Sodium in our body ): in the blood occurs whenever there is excess sodium in relation to water. There are numerous causes of hypernatremia; these may include kidney disease, too little water intake, and loss of water due to diarrhea and/or vomiting. • Hyponatremia: A decreased concentration of sodium occurs whenever there is a relative increase in the amount of body water relative to sodium. This happens with some diseases of the liver and kidney, in patients with congestive heart failure.

  10. Potassium (K+ ) • Potassium is the major positive ion (cation) found inside of cells • Increased potassium is known as hyperkalemia. Potassium is normally excreted by the kidneys, so disorders that decrease the function of the kidneys can result in hyperkalemia. Certain medications may also predispose an individual to hyperkalemia. • Hypokalemia, or decreased potassium, can arise due to kidney diseases; excessive loss due to heavy sweating, vomiting, or diarrhea, eating disorders, certain medications, or other causes.

  11. Calcium (Ca2+ ) • Calcium regulates muscle contraction, including the heartbeat. It also plays a key role in normal blood coagulation (clotting). • Nearly all of the calcium in our bodies is stored in our teeth and bones, where it supports their hardness and structure.

  12. Hypercalcemia: flank pain, muscle tone,mental confusion, impaired memory, slurred speech • Hypocalcemia: convulsions, muscle cramps, tingling of fingertips, ears, nose, toes, tetany

  13. Chloride(Cl-) • Chloride is the major anion (negatively charged ion) found in the fluid outside of cells and in the blood • Increased chloride (hyperchloremia): Elevations in chloride may be seen in diarrhea, certain kidney diseases, and sometimes in over activity of the parathyroid glands.   • Decreased chloride (hypochloremia): Chloride is normally lost in the urine, sweat, and stomach secretions. Excessive loss can occur from heavy sweating, vomiting, and adrenal gland and kidney disease

  14. Magnesium(Mg2+ ) • Magnesium (Mg) is the second most abundant intracellular cation and is a cofactor in more than 300 enzymatic reactions involving energy metabolism and protein and nucleic acid synthesis • Approximately half the total Mg in the body is present intracellularly in soft tissue, and the other half is present in bone. Less than 1% of the total body Mg is present in blood

  15. Hypermagnesemia: Too much magnesium. This is a rare disorder that can occur in people with Addison’s disease and end-stage renal disease. • Hypomagnesemia: Too little magnesium. Causes include: chronic alcoholism; malnutrition; malabsorption issues; digestive system disorders; chronic diarrhea; excessive sweating; medications like diuretics and cyclosporine; and certain antibiotics.

  16. Phosphate (PO43-) • Helps maintain body's acid base balanceInvolved in important chemical reactions in the bodyNecessary for many B vitamins to be effectiveHelps promote nerve and muscle actionPlays role in carbohydrate metabolismImportant for cell division and for the transmission of hereditary traits

More Related