A solution containing 1.66 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)

A 31.00 mLmL sample of an H2SO4H2SO4 solution of unknown concentration is titrated with a 0.1372 MM KOHKOH solution. A volume of 41.22 mLmL of KOHKOH was required to reach the equivalence point. What is the concentration of the unknown H2SO4H2SO4 solution?

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 0.95 M NaH2PO4 and 0.68 M Na2HPO4. H2PO4-  + H2O ⇌  HPO42-  + H+  pKa= 7.21  (5 marks total) a. From the reaction above indicate the weak acid and the conjugate base involved in making this buffer. (2 marks) b. Calculate the pH of the phosphate buffer solution. Provide your answer with 2 decimal places (2 marks) c. 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? (1 mark)

If a 8.70 mL aliquot of acetic acid (HCH3COO) needs 11.05 mL of 0.080M Ca(OH)2 to reach the equivalence point, what is the concentration of the acetic acid?

A sample of a certain monoprotic weak acid was dissolved in water and titrated with 0.150 M NaOH, requiring 16.00 mL to reach the equivalence point. During the titration, the pH after adding 4.00 mL NaOH was 6.912. Calculate Ka for the weak acid.

A certain weak acid, HAHA, with a KaKaK_a value of 5.61×10−65.61×10−6, is titrated with NaOHNaOH. A solution is made by titrating 8.00 mmolmmol (millimoles) of HAHA and 1.00 mmolmmol of the strong base. What is the resulting pH?   More strong base is added until the equivalence point is reached. What is the pH of this solution at the equivalence point if the total volume is 47.0 mL ?

A student performs a titration, titrating 25.00 mL of a weak monoprotic acid, HNO2, with a 1.506 M solution of NaOH. They collect data, plot a titration curve and determine that the equivalence point was reached after the addition of 27.66 mL of the base.  What is concentration of NO2- at equivalence point (in M)?

A titration of 79.0 mL of a tartaric acid (H₂C₄H₄O₆) solution of unknown concentration with 0.805 M LiOH requires 32.0 mL to reach the second equivalence point. What is the concentration of the tartaric acid solution?

Calculating the pH of a weak base titrated with a strong acid 0/5 Izabella An analytical chemist is titrating 165.0 mL of a 0.7400M solution of methylamine (CH3NH2) with a 0.4100M solution of HNO3. The pK of methylamine is 3.36. Calculate the pH of the base solution after the chemist has added 318.6 mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO 3 solution added. Round your answer to 2 decimal places. pH = ☐ ☑ ? 18 Ar

A solution containing 1.87 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)