Acid

Formula               Acid Name          Salt Name              anion

HF                     Hydrofluoric Acid     Hydrofluorate    HF (aq)      <----> H + F

H + HCl           Hydrochloric Acid    Hydrochlorate      HCl (aq)       ----> H + Cl

HBr                   Hydrobromic Acid  Hydrobromate     HBr (aq)       ----> H + Br

HI                       Hydroiodic Acid      Hydroiodate         HI (aq)          ----> H + I

HCN                 Hydrocyanic Acid    Hydrocyanate      HCN (aq)    <----> H+ CN

H2S                 Hydrosulfuric Acid  Hydrosulfate        H2S (aq)     <----> H + S

HNO2                   Nitrous Acid        Nitrite                   HNO2 (aq)  <----> H + NO2

HNO3                  Nitric Acid              Nitrate                    HNO3 (aq)    ----> H + NO3

H2SO3              Sulfurous Acid        Sulfite                   H2SO3 (aq) <----> H2O+SO2

H2SO4                Sulfuric Acid          Sulfate                  H2SO4 (aq)   ----> H + HSO4

H3PO3          Phosphorous Acid   Phosphite             H3PO3 (aq) <----> 3H + PO3

H3PO4            Phosphoric Acid      Phosphate            H3PO4 (aq) <----> 3H + PO4

H2CO3               Carbonic Acid        Carbonate            H2CO3 (aq) <----> 2H +CO3

HClO               Hypochlorous Acid Hypochlorite        HClO (aq)    <----> H + ClO

HClO2                Chlorous Acid        Chlorite                                 HClO2 (aq)  <----> H + ClO2

HClO3                   Chloric Acid          Chlorate                HClO3 (aq)  <----> H + ClO3

HClO4              Perchloric acid      Perchloorate           HClO4 (aq)  <----> H + ClO4

HBrO           Hypobromous Acid   Hypobromite        HBrO (aq)   <----> H + BrO

HBrO2                Bromous Acid       Bromite                   HBrO2 (aq) <----> H + BrO2

HBrO3                 Bromic Acid          Bromate                HBrO3 (aq) <----> H + BrO3

HBrO4             Perbromic acid      Perbromate          HBrO4 (aq) <----> H + BrO4

HIO                   Hypoiodous Acid   Hypoiodite            HIO (aq)      <----> H + IO

HIO2                    Iodous Acid          Iodite                     HIO2 (aq)      <----> H + IO2

HIO3                     Iodic Acid              Iodate                    HIO3 (aq)      <----> H + IO3

HIO4                    Periodic Acid        Periodate              HIO4 (aq)      <----> H + IO4

Reaction Quotient

         If a reaction mixture, containing both reactants and products, is not at equilibrium ; how can we determine in which direction it will proceed. The answer is to compare the current concentration ratios to the equilibrium constant. The concentration ratio of the products ( raised to the power of their coefficients ) to the reactants ( raised to the power of their coefficients) is called the reaction quotient, Q.

Q > K = go backward

Q < K = go forward

Q = K = at equilibrium

Q = 0 = go forward

Q = infinity = go backward

Video From : http://www.youtube.com/watch?v=60Sylqei2DY

Heat Transfer

Convection is the transfer of heat by the actual movement of the warmed matter. Heat leaves the coffee cup as the currents of steam and air rise. Convection is the transfer of heat energy in a gas or liquid by movement of currents. (It can also happen is some solids, like sand.) The heat moves with the fluid. Consider this: convection is responsible for making macaroni rise and fall in a pot of heated water. The warmer portions of the water are less dense and therefore, they rise. Meanwhile, the cooler portions of the water fall because they are denser.

Conduction is the transfer of energy through matter from particle to particle. It is the transfer and distribution of heat energy from atom to atom within a substance. For example, a spoon in a cup of hot soup becomes warmer because the heat from the soup is conducted along the spoon. Conduction is most effective in solids-but it can happen in fluids. Fun fact: Have you ever noticed that metals tend to feel cold? Believe it or not, they are not colder! They only feel colder because they conduct heat away from your hand. You perceive the heat that is leaving your hand as cold.

Radiation: Electromagnetic waves that directly transport ENERGY through space. Sunlight is a form of radiation that is radiated through space to our planet without the aid of fluids or solids. The energy travels through nothingness! Just think of it! The sun transfers heat through 93 million miles of space. Because there are no solids (like a huge spoon) touching the sun and our planet, conduction is not responsible for bringing heat to Earth. Since there are no fluids (like air and water) in space, convection is not responsible for transferring the heat. Thus, radiation brings heat to our planet.

https://www.nc-climate.ncsu.edu/edu/k12/.conduction

From : http://www.mansfieldct.org/schools/mms/staff/hand/convcondrad.htm

Equilibrium Constants for Reactions Involving Gases

The concentration of a gas in a mixture is proportional to its partial pressure. Therefore, the equilibrium constant can be expressed as the ratio of the partial pressures of the gases.

Reference : http://scienceaid.co.uk/chemistry/physical/eqconstants.html

Reference : http://chem-guide.blogspot.com/2010/04/relation-between-kp-and-kc-derivation.html

In calculation K_p, the partial pressures are always in atm. The substances that are not in form of gas are not use to calculate for K_p. And the relationship between them will be shown below.

Reference : http://chem-guide.blogspot.com/2010/04/relation-between-kp-and-kc-derivation.html

**is the difference between the number of moles of reactants and moles of products.

**Notice : K_p and K_c are not necessarily the same. And they will be the same when  = 0.

 

Video From : http://www.youtube.com/watch?v=pnZpn9N8XbU

Relationships Between K And Chemical Equation

1)    When the reaction is written backward, the equilibrium constant is inverted.

                                             

2)    When the coefficients of an equation are multiplied by a factor, the equilibrium constant is raised to that factor.

3)    When you add equations to get a new equation, the equilibrium constant of the new equation is the product of the equilibrium constants of the old equations.

4)    When you subtract equations to get a new equation, the equilibrium constant of the new equation is the quotient of the equilibrium constants of the old equations.