Determine the concentration of h 3 o + to the correct number of significant figures in a solution with each ph. describe how these calculations show the relationship between the number of digits to the right of the decimal place in ph and the number of significant figures in concentration. ph = 2.50 ph = 2.51 ph = 2.52

To calculate the concentration of H3O+

1- when PH = 2.5 :

The explanation:

we are going to use this formula:

PH = - ㏒[H3O+]

and we here have PH = 2.5 so, by substitution:

2.5 = -㏒ [H3O+]

∴ [H3O+] = 0.00316 ≈ 0.003

2- when PH = 2.51 :

The explanation:

we are going to use this formula:

PH = - ㏒[H3O+]

when here we have PH = 2.51 so, by substitution:

2.51 = - ㏒[H3O+]

∴[H3O+] = 0.00309 ≈ 0.003

3- when PH = 2.52 :

The explanation:

we are going to use this formula:

PH = - ㏒[H3O+]

when here we have PH =2.52 so, by substitution:

2.52 = -㏒[H3O+]

∴[H3O+] = 0.00301 ≈ 0.003

we can see that when the the number of digits to the right of the decimal place in ph increase, the number of significant figures in concentration decrease.

adding or remove a gaseous reactant or product changes the concentrations. if the concentration of reactant or product is increased, the system will shift away from the side in which concentration was increased (i.e. if the concentration of reactants is increased, the system will shift toward the products. if more products are added, the system will shift to form more reactants). conversely, if the concentration of reactant or product is decreased, the system will shift toward the side in which concentration was decreased (i.e. if reactants are removed, the system will shift to form more reactants. if the concentration of products is decreased, the equilibrium will shift toward the products).

explanation:

"hydrogen bonding is the attraction of h atoms in the water molecule (slight + charge) to o atoms in a neighboring water molecule (slight - charge); it is a weak interatomic force. but it is still strong enough to the water molecules "stick" together."