# Question:Can you please help me with part a, b, & c based on the information below:242Acid: Na24 *2pH= 8.00

Base: NaH_{}PO_{} * H_{}O = 137.99 g/mol

_{}HPO_{} 7H_{}O = 268.07 g/mol

Conc (M) =0.100

8.0=7.21+Log[A/B]

0.79=Log[A/B] -> 10^{0.79}=B/A -> 6.16595=B/A -> B=6.16595A

0.01mol= A+6.16595

0.01mol= 716595

Acid = 0.1925 g

Base = 2.30 g

Solids (acid & base) were added to a 100ml volumetric flask and filled with DI water to the 100mL mark

**a) Calculate the theoretical pH of the buffer solution after the addition of 1.00mL of 0.100M** **NaOH ;added to 100.00ml of buffer solution**

**b) Calculate the theoretical pH of the buffer solution after the addition of 1.00mL of 0.100M HCl**

**c) Calculate the theoretical values for the pH of the NaOH and HCl solutions made in water**

-1.00mL of 0.100M NaOH added to 50.0mL of DI water - pH: 11.11

-1.00ml of 0.100M of HCl to 50mL of DI water - pH: 2.56

**i. You will need to know the concentration of NaOH an HCl once they were added to the water in each solution.**

**ii. You will then need to know that HCl and NaOH are** **strong** **acid and base, respectively, which means they will dissociate completely in water**

**iii. You can then** **determine** **the [H**^{+}**] concentration (or[OH**^{-}**]... then the [H**^{+}**]) and calculate pH**

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