A 0.8746 g sample of an unknown acid, HA, is reacted with NaOH (aq). The reaction that occurs is as follows: HA (aq) + NaOH (aq) =====> NaA (aq) + H2O (l) If the complete reaction of the HA sample requires exactly 28.62 mL of 0.1927 M NaOH (aq), what is the molecular mass of HA ?
A 0.8746 g sample of an unknown acid, HA, is reacted with NaOH (aq). The reaction...
15. (6 pts.) You have 0.669 g of an unknown acid, HA which reacts with NaOH according to the balanced chemical equation HA(aq) + NaOH(aq) - NaA(n) + H2O() If 36,04 ml. of 0.509 M NaOH is required to titrate the acid to the equivalence point, what is the molar mass of the acid?(4 pts.) Identify the acid (2 pts.)
A 0.704 g of a pure acid, HA, is dissolved in water and an acid-base indicator added. The solution requires 33.78 mL of 0.256 M NaOH solution to reach the end point. What is the molar mass of the acid? HA(aq) + NaOH(aq) LaTeX: \longrightarrow⟶ NaA(aq) + H2O(aq) Group of answer choices 81.4 g/mol 199 g/mol 145 g/mol 20.0 g/mol
1. Calculation of pH. A weak acid HA (pKa = 4.85) reacted with strong base NaOH The reaction is HA + NAOH H20 + NaA. There are 100 mL 0.100 M HA solution, and the concentration of Na OH is 0.100 M. 0 moles a. What is the pH when 0.00 mL of NaOH is added to the 100 mL HA solution? 2 x1 les b. What is the pH when 20.0 mL of NaOH is added to the 100...
show all work Consider that 20.0 mL of 0.10 M HA (an arbitrary weak acid, Ka= 2.5 × 10−6) is titrated with 0.10 M NaOH solution. The ionization of HA in water occurs as the following. HA (aq) + H2O(l) ⇌ A (aq) + H3O (aq) The neutralization reaction between HA and NaOH can be expresses as the following. HA (aq) + NaOH (aq) NaA (aq) + H2O (l) Answer the following questions. A) What will be the initial...
A 35.0 mL sample of an unknown HC104 solution requires 43.3 mL of 0.102 M NaOH for complete neutralization. Part A What was the concentration of the unknown HC104 solution? The neutralization reaction is: HC1O4 (aq) + NaOH(aq) +H2O(l) + NaClO4(aq) O 2 ? Submit Request Answer Provide Feedback Next >
A 0.704 g of a pure acid, HA, is dissolved in water and an acid- base indicator added. The solution requires 33.78 mL of 0.256 M NaOH solution to reach the end point. What is the molar mass of the acid? HA(aq) + NaOH(aq) → NaA(aq) + H2O(aq) 145 g/mol 81.4 g/mol 20.0 g/mol 199 g/mol Based on the equation below, which is correct? 2 C2H2(g) + 5 O2(g) → 4 CO2(g) + 2 H2O(g) C2H2(g) is reduced O2(g) is...
We dissolve 2.77 g of an unknown acid, HA, in enough water to produce 25.0 mL of solution. The pH of this solution of HA(aq) is 1.33. We titrate this solution with a 0.250 M solution of NaOH. It takes 41.1 mL of the NaOH solution to reach the equivalence point.What is the molar mass of HA and What is the pKa value of HA(aq)?
A 35.0 mL sample of an unknown HCIO4 Solution requires 50.3 mL of 0.109 M NaOH for complete neutralization. What was the concentration of the unknown HCIO, solution? The neutralization reaction is: HCIO,(aq) + NaOH(aq) →H2O(l) + NaC104(aq) 0 21 ? Submit Previous Answers Request Answer Part C 0.0400 mol of glucose in 89.3 mL of solution Express your answer using three significant figures. V AZO + O 2 ?
A 0.5220 −g sample of an unknown monoprotic acid was titrated with 9.94×10−2 M NaOH. The equivalence point of the titration occurs at 23.86 mL . Determine the molar mass of the unknown acid.
We dissolve 2.77 g of an unknown acid, HA, in enough water to produce 25.0 mL of solution. The pH of this solution of HA(aq) is 1.33. We titrate this solution with a 0.250 M solution of NaOH. It takes 41.9 mL of the NaOH solution to reach the equivalence point. (a) (2 points) What is the molar mass of HA? (b) (2 points) What is the pKa value of HA(aq)? (c) (2 points) What is the pH at the...