Some amount of a diprotic acid is dissolved in 100 mL of H20. 70.0 mL of 0.100 M NAOH is added to reach the second equivalence point. What was the molarity of the acid solution that was made?

of 15 > The identity of an unknown monoprotic organic acid is determined by titration. A 0.300 g sample of the acid is titrated with 0.103 M NaOH. What is the molar mass of the compound if 16.2 mL of the NaOH solution is required to neutralize the sample? molar mass: The compound is 60.0% C, 4.48% H, and 35.5% O. What is the molecular formula of the organic acid? formula: $ 4 C R F LL dº 5 % V T G 6 MacBook Pro B Y H & 7 N * 00 8 J 1 M ( 9 K O 1 L command P A. : i { option [ + 11 = ? mol 1

For a titration of HCl with NaOH, 3.0 mL of 0.4 M NaOH are needed to neutralize 4.0 mL of the HCI. What is the molarity of the HCI? O 960 M O 0.15 M O .3 M O .0096 M

1. How do you prepare a 100mL of 0.1 M phosphate buffer?To make 100 mL of 0.1 M phosphate buffer: Calculate the amount of sodium phosphate needed. moles of sodium phosphate = (0.1 mol/L) x (0.1 L) = 0.01 moles mass of sodium phosphate = moles x molar mass = 0.01 moles x 142 g/mol = 1.42 g Dissolve 1.42 g of sodium phosphate in distilled water in a 100 mL volumetric flask. Adjust the pH of the solution to the desired value (usually around 7.4) using a strong acid or strong base. Bring the solution to the final volume (100 mL) with distilled water.   2. From the anterior buffer, how do you make 100mL of 0.05 M? To make 100 mL of 0.05 M phosphate buffer from the 0.1 M stock solution: Calculate the amount of the 0.1 M phosphate buffer needed. moles of phosphate buffer = (0.05 mol/L) x (0.1 L) = 0.005 moles Calculate the volume of the 0.1 M phosphate buffer needed. moles = concentration x volume (in liters) volume = moles / concentration = 0.005 moles / 0.1 mol/L = 0.05 L or 50 mL Measure…

A 0.258-g sample of a pure triprotic acid, H3A, (where A is the generic anion of the acid), was dissolved in water and titrated with 0.150 M barium hydroxide solution. The titration required 13.9 mL of the base to reach the equivalence point. What is the molar mass of the acid? 227 g/mol 82.5 g/mol 371 g/mol 124 g/mol 186 g/mol

Use the References to access important values if needed for this question. Which of the following aqueous solutions are good buffer systems? 0.28 M ammonia + 0.35 M calcium hydroxide . 0.11 M potassium hydroxide + 0.23 M potassium bromide . 0.39 M sodium perchlorate + 0.23 M potassium perchlorate . 0.15 M hypochlorous acid + 0.13 M potassium hypochlorite . 0.27 M hydroiodic acid + 0.25 M potassium iodide .

7. A solution was made by mixing 50.0 mL of 0.750 M HCN with 25.0 mL of water. What is the pH of this solution? The pka of HCN = 9.31. 8. One of the compounds featured on the TV series "Breaking Bad" was hydrofluoric acid (HF), pKa = 3.14. a) A solution of HF has a pH = 1.77. What was the initial [HF] for this solution in mol L-1? b) What is the equilibrium concentration of F in this solution in mol L-1? c) What is the percent ionization of HF in this solution?

A 28.00 mLmL sample of an H2SO4H2SO4 solution of unknown concentration is titrated with a 0.1422 MM KOHKOH solution. A volume of 43.22 mLmL of KOHKOH was required to reach the equivalence point. What is the concentration of the unknown H2SO4H2SO4 solution?         Express your answer using four significant figures.

b A chemistry graduate student is given 300. mL of a 1.20M pyridine (CHN) solution. Pyridine is a weak base with K₂= 1.7 × 10 What mass of CH₂NHCl should the student dissolve in the C-H₂N solution to turn it into a buffer with pH = 5.20? You may assume that the volume of the solution doesn't change when the C5H₂NHCl is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. 0 x10 I 5