You will prepare 5 cuvettes with different concentration of sodium phosphate (Pi) using the stock 1mM Pi, 0.5mM PNPP solution (in water) and 0.2M Tris-HCl, pH=8.00. For this part, the concentration of PNPP will remain constant at 0.05mM. Fill the table below (before coming to lab) and use it to prepare your cuvettes. Your blank for each reaction is the PNPP mixed with Tris-HCL and Pi. DO NOT ADD ENZYME AT THIS POINT!!! Final [Pi] uM Volume of 1mM Pi Final [PNPP] mM Volume of 0.5mM PNPP Volume of 0.2M Tris-HCl (uL) Volume of enzyme (uL) Total Volume (uL) 0   0.05     100 1500 3.33   0.05     100 1500 20   0.05     100 1500 50   0.05     100 1500 100   0.05     100 1500

Help! Please solve Q5 all parts

5. What would be the pH of a 100.0 mL solution containing 0.24 M formic acid (HCHO2; Ka = 1.8x10-4) and 0.24 M sodium formate (NaCHO₂)?

A group of students perform a titration experiment. The buret tube is filled to the 0.00ml line with 0.100M NaOH solution. The E. flask contains 50.0ml ov 0.100M HC2H3O2 solution. The Ka of the acetic acid is: Ka = 1.8 x 10-5. A) Write the ionic equation for the conjugate acid reactihng with water. One product is the OH- polyatomic ion.  B) What is the pH of the equivalence point?

Determine the pH of a solution that is prepped with 0.25 M CH3NH3Cl and 0.15 M CH3NH2  (Kb = 3.7 x 10-4) Thank you!

Correct answers are given!!! Please just show me how to get them.

Calculate the pH of a 1 L solution containing 10 mL of 2 M acetic acid (pKa = 4.75) and 5 g of sodium acetate (formula weight = 82 g/mol). Be sure to show your work and to include the appropriate units in your calculations.

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20. Calculate the pH (aqueous, 25°C) of 0.545 M HCOOH mixed with 0.628 M HCOOK in a total of 250.0 mL, AFTER 5.000 mL of 5.00 M LiOH have been added. (For HCOOH, K₁ = 1.80 × 10-4) (You MUST show your work).