Now you use the above standardization NaOH (0.0702mol/L) to titrate a 25.0mL aliquot of H2SO4. It takes 12.0mL of your standardized NaOH to come to the equivalent point. Calculate the molarity of H2SO4

You are titrating 30 mL of 0.100M H3PO4 with 0.200 M KOH. For H3PO4: Ka1=1.1X 10-², Ka2 = 7.5 X 10-8, and Ka3 = 4.8 X 10-¹3. What is the pH after you add 35.00 mL of KOH?

= く O Acids and Bases Calculating the composition of a buffer of a given pH 0/5 a A chemistry graduate student is given 300. mL of a 0.70 M hydrocyanic acid (HCN) solution. Hydrocyanic acid is a weak acid with K = 4.9 x 10 10. What mass of NaCN should the student dissolve in the HCN solution to turn it into a buffer with pH = 9.48? You may assume that the volume of the solution doesn't change when the NaCN is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. x10 ㅁ

A buffer with pH = 8.96 must be created. 8.90 g of the acid component of the best buffer system will be used, and the volume of the solution will be 1 L. Choose which is the best buffer system, then compute the mass of the salt or base component of the chosen system.   Choices:  HClO (Ka = 2.9 x 10-8 , 52.46 g/mol)& KClO (90.55 g/mol)  NH3 (Ka = 5.65 x 10-10 , 17.031g/mol) &NH4Cl (53.491 gmol) CH3COOH (Ka = 1.77 x 10-5 , 60.052 g/mol) & CH3COOK (98.15 g/mol) HClO2 (Ka = 1.1 x 10-2 , 68.46 g/mol)) & KClO2 (106.55 g/mol)

What is the [H3O+] and the pH of a benzoic acid-benzoate buffer that consists of 0.13 M C6H5COOH and 0.30 M C6H5COONa? (Ka of benzoic acid = 6.3 × 10−5)  Be sure to report your answer to the correct number of significant figures. [H3O+] = ___× 10___MpH =____

A 100.0 mL buffer solution is 0.110 mol L-¹ in CH3NH2 and 0.130 mol L-¹ in CH3NH₂Br. Part A What mass of HCI will this buffer neutralize before the pH falls below 9.55? ( Kb (CH3NH₂) = 4.40 × 10-4) Express the mass in grams to two significant figures. mun shummu za

0.1988g of an unknown solid acid is combined with 50ml of deionized water. 15.5ml of NaOH with a 0.2 concentration is combined in a titration. what is the unknown solid diprotic acid?

End Points in Strong-Base Titration of Mixed Strong Monoprotic and Weak Polyprotic Acids 1.39×10-2; ka2 = 6.73×10−8) is titrated A mixed aqueous solution of HCl and sulfurous acid (H₂SO3; Kal with 0.1000-M NaOH. The first end point (ethyl orange indicator) is reached after 38.91 mL of NaOH has been added. The second end point (thymolphthalein indicator) is reached after a total of 54.79 mL of NaOH has been added. What quantity of HCI (units of mol or mmol) was present in the initial mixture? 2.303 mol Submit Answer Incorrect. Tries 2/5 Previous Tries What quantity of sulfurous acid (units of mol or mmol) was present in the initial mixture? 1.59 mol

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…

Select the answer that best describes the experimental setup of the titration curve shown in the image below 12 Hd H] 8 4 0 10 volume of titrant (mL) 20 20 strong base (beaker) and strong acid (burette) weak base (beaker) and strong acid (burette) weak acid (beaker) and strong base (burette) strong acid (beaker) and strong base (burette)