A solution containing 1.22 g of a diprotic acid H₂C₃H₂O₄ (malonic acid) was titrated with 45.5 mL of NaOH to reach the second equivalence point. What is the concentration of the NaOH solution? (MW_malonic acid = 104.06 g/mol)

When 30 .00 mL of 0.1011 M HCl in 50 mL of deionized water is titrated against 0.09889 M NaOH, the pH increases. What is the volume (in mL) of NaOH required to reach the equivalence point and a pH of 7.00? Find the pH when the volume of NaOH added is 0.02 mL less than the volume required to reach the equivalence point. Find the pH when the volume of NaOH added is 0.01 mL less than the volume required to reach the equivalence point. Find the pH when the volume of NaOH added is 0.02 mL more than the volume required to reach the equivalence point. Comment on the significance of the changes in pH values in relation to the increments of sodium hydroxide added when going “through” the end point. Define equivalence point. For a weak base/strong acid titration, is the pH at the equivalence point <, >, or equal to 7?

Question 6 Type numbers in the boxes. 45.0 mL of o.650 M HNO, is titrated by 0.650 M KOH. aby Part 1: 10 points Calculate the pH of the acid solution before any titrant is aby Part 2: 10 points added. aby Part 3: 1 points pH = aby Part 4: 10 points Calculate the pH after 1.47 mL of o.650 M KOH is added 31 points to 45.0 mL of 0.650 M HNO,. pH = Calculate the pH after 45.00 mL of o.650 M KOH is added to 45.0 mL of o.650 ΜΗΝΟ. pH = Calculate the pH after 89.5 mL of o.650 M KOH is added to 45.0 mL of 0.650 M HNO,- pH =

For humans to maintain the pH of their blood close to 7.4, the body uses three buffer systems: carbonate, phosphate and proteins. If the pH of the blood goes below 6.8 or above 7.8, death may result. Imagine you want to make a phosphate buffer in the lab that resembles the bloods phosphate buffer. You start by mixing 1.0 M NaH2PO4 and 0.50 M Na2HPO4. H2PO4-  + H2O ⇌  HPO42-  + H+         pKa= 7.21 From the reaction above indicate the weak acid and the conjugate base involved in making this buffer. Calculate the pH of the phosphate buffer solution. Provide your answer with 2 decimal places. If the pH calculated in b. was the blood pH of an actual patient, would you say this patient’s blood pH is in the normal range or are they suffering from alkalosis or acidosis?

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

The following diagrams contain one or more of the compounds: H2A, NaHA, and Na2A, where H2A is a weak diprotic acid. Which solution is the most effective buffer solution? Water molecules and Na+ ions have been omitted for clarity. = H2A НА = A2- %3D (a) (b) (c) (d) b.

A certain indicator, HA, has a K value of 2.0 x 10. The protonated form of the indicator is blue and the ionized form is red. What is the pK, of the indicator? pK = What is the color of this indicator in solution with pH = 3? about us careers privacy policy terms of use contact us help 949 PM XI 风下 3/10/202 edts f12 inse ho 立

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 =____

In a titration of 73.0 mL of a 0.500 M solution of a diprotic acid H.C.H.O. (malonic acid) with 0.255 M NaOH, how many grams of NaOH are required to reach the second equivalence point? (MW_NaOH = 39.997 g/mol) B

Consider the titration of an acetic acid (CH3COOH) with sodium Hydroxide  to form sodium acetate (NaCH3COO) and water. A 10.0 ML sample of acetic acid requires 37.55 ML of 0.233 M NaOH to reach the equivalence point. The amphiprotic substance is acting as :  Neutral an acid Or a base