Answered: A 25.0 mL sample of 0.200 M HCO2H(aq)…

A 25.0 mL sample of 0.200 M HCO2H(aq) is titrated with 0.100 M KOH(aq). What is the pH at the equivalence point? (Ka of HCO2H = 1.8 × 10-4) 8.28 O 8.52 O 7.00 O 10.26 5.71

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter14: Acid-base Equilibria

Section: Chapter Questions

Problem 98E: Calculate the pH of a buffer solution prepared from 0.155 mol of phosphoric acid, 0.250 mole of...

See similar textbooks

Related questions

Q: Calculate the pH of the resulting solution when 30.0 mL of 0.16 M KOH are added to 46.0 mL of 0.15 M…

A: Given, Volume of solution = 30.0ml Molarity of KOH = 0.16M Volume of HClO = 46.0ml Molarity of HClO…

Q: In a titration experiment of a 25.00 ml of 0.100 M CH3CO2H with 0.100M NaOH, 12.50 mL of NaOH were…

A: We have 25 mL of 0.1 M acetic acid and 0.1 M 12.5 ml NaOH , we have to calculate the pH of resulting…

Q: Sodium acetate, NaCH;COO (82.0343 g/mol) is commonly used as acidic buffer solution. Estimate the…

Q: What is the pH when 66.6 mL of 0.25 M HNO2 is titrated with 54.3 mL of 0.35 M NaOH?

A: Given:Molarity of HNO2 is M1=0.25 Mvolume of HNO2 is V1=66.6ml or 0.066LMolarity of NaOH is…

Q: A 25mL sample of a 0.15M solution of a weak acid Ka=3.0x10^-6 is titrated ith 0.15M NaOH. What is…

A: Calculate the number of moles of weak acid and the strong base NaOH. The number of moles can be…

Q: b) A buffer solution is prepared by adding 40.0 g of sodium acetate CH;COONA to 500 mL of a 0.200 M…

A: Given: Mass of CH3COONa =40.0g Molar mass of CH3COONa =82.03 g/mol Volume of solution =500ml=0.5 L…

Q: 20. mL of 0.25 M of HC2H3O2 is titrated with 0.40 M KOH, Calculate the pH of the solution after 15…

Q: 45.0 mL of 1.023 M HCOOH is titrated with 0.740 M LiOH. What is the pH after 30.0 mL of LiOH has…

A: pH is used to determine the concentration of hydronium ion.

Q: K, of a weak acid HX is 2.16 x 10-6. During a titration, an analyte solution containing a mixture of…

A: The Henderson Hasselbalch equation is given by, pH = pKa + logsaltacid where Ka is the acid…

Q: 10.5 mL of 0.10M HF (ka+6.3x10-4) is titrated with 5.7 mL of 0.10M NaOH. What is the pH of the…

A: Moles of HF = (10.5*0.1)/1000 = 0.00105 Moles of NaOH = (5.7*0.1)/1000 = 0.00057 NaOH and HF will…

Q: Which of the following will raise the pH of a strong acid HA in aqueous solution? I addition of…

A: I) Since HA is a strong acid hence it will dissociate completely into H+ and A- ions And since pH =…

Q: What is the pH of a 80.0 mL solution of 1.25 M concentration acid HA after 40.0 mL of 2.00 M…

A: Equation for the reaction of the monoprotic acid, HA and NaOH is: HA(aq) + NaOH(aq) ---->…

Q: 1. A 25.00 mL solution of 0.0920 M HNO3 was titrated with 0.00, 15.00, 23.00, and 30.00 mL of 0.1000…

A: The titration reaction will be as follows: HNO3 + KOH ------------> KNO3 + HOH. The volume of…

Q: 40.00 mL of a 0.30 M HCI solution is titrated with 0.35 M NaOH. What is the pH of the solution after…

A: By definition molarity is, molarity=number of moles of solutevolume of solution in L The molarity of…

Q: A buffer solution is prepared by dissolving 1.50g each of benzoic acid (MM=122.1, Ka=6.3 x 10^-5),…

A: Given, Mass of benzoic acid (HC7H5O2) = 1.50g Molar mass of benzoic acid =122.1g/mol Mass of sodium…

Q: At 22 °C, an excess amount of a generic metal hydroxide, M(OH),, is mixed with pure water. The…

Q: A 25.00-mL solution of 0.100 M HCl is titrated with 0.150 M NaOH. What is the pH after 18.00 mL of…

Q: Calculate the pH of a buffer made from mixing 11.0 mL of 0.421 M NaC2H3O2 and 12.5 mL of 0.305 M…

A: Given: The volume of NaC2H3O2 = 11.0 mL The concentration of NaC2H3O2 =0.421 M The volume of HC2H3O2…

Q: Please answer 1A, 1B, 1C, and 1D

A: Hello. Since your question has multiple sub-parts, we will solve first three sub-parts for you. If…

Q: KOH is used to titrate an acid to the equivalence point. The indicator thymolphthalein was chosen as…

A: The chemical indicator is any substance which gives visible sign, usually by colour change, of the…

Q: In the titration of 70.0 mL of a 0.300 M HF with 0.300 M KÖH, calculate the pH: (a) after 35.0 mL of…

A: we need to calculate the pH for the titration of KOH with HF

Q: 1. The pH of a buffer solution containing 0.5 mole/litre of CH:COOH and 0.5 mole/litre CH.COONA has…

Q: Twenty-five milliliters of 0.10 M HCl(aq) is titrated with 0.10 M NaOH(aq). What is the pH at…

A: The pH at the equivalence point has to be identified.

Q: A 25.0-mL sample of 0.150 M hydrazoic acid is titrated with a 0.150 M NaOH solution. What is the pH…

A: The explanation is given below-

Q: How much (in grams) Na2HPO4 must be added to 100 mL 1.0 M NaH2PO4 solution to prepare a buffer…

Q: A buffer solution is prepared from equal volumes of 0.200 M acetic acid and 0.600 M sodium acetate.…

A: Given: Concentration of acetic acid i.e. CH3COOH = 0.200 M Concentration of sodium acetate i.e.…

Q: What is the pH of a buffer prepared by mixing 100 ml 0.050 mM NaH2PO4 and 25 ml 0.075 mM NɑżHPO4?…

A: Given, Molarity of NaH2PO4 (acid) = 0.050 mM Volume of NaH2PO4 (acid) = 100 mL Molarity of…

Q: A144L buffer solution consists of 0320M propanoic acid and 0.189 M sodium propanoate. Calculate the…

A: Interpretation: A 1.44 L buffer solution consists of 0.320 M propanoic acid and 0.189 M sodium…

Q: A 25.0 mL sample of 0.150 M benzoic acid is titrated with a 0.150 M NAOH solution. What is the pH…

A: In this question, we have to find out the correct answer of given problem by the help of the…

Q: What mass (in g) of sodium formate, HCOONA, must be added to 10.0 L of a 0.483 Maqueous solution of…

Q: What volume in mL of 0.2572 M NaOH must be added to 500.0 mL of 0.1000 M chlorous acid (HClO2, Ka =…

A: Given: pH = 2.25 Concentration of HClO2 = 0.100 M Volume of HClO2 = 500.00 mL Concentration of NaOH…

Q: If 50.00 ml of 1.00M HC,H,O; (K, = 1.8 x 10*) is titrated with 1.00 M NaOH. What is the pH of the…

A: Volume of CH3COOH = 50ml Concentration of CH3COOH = 1M Concentration of NaOH = 1M Ka = 1.8×10-5 We…

Q: How many grams of NaF (41.98817 g/mol) would have to be added to 2.00 L of 0.100 M HF (20.01 g/mol)…

Q: 15. A 25.0 mL solution of 0.250 mol/L methanoic acid, HCOOH(aq), is titrated with a 0.100 mol/L…

Q: A 25.00 mL solution of 0.0920 M HNO3 was titrated with 0.00, 15.00, 23.00, and 30.00 mL of 0.1000 M…

A: Molarity of HNO3 = 0.0920 M Volume of HNO3 = 25.00 mL = 25.00 / 1000 L = 0.025 L Molarity of KOH =…

Q: What pH would be measured from a solution that is made by mixing 100.0 mL of 0.050 M NaC2H3O2 and…

Q: Calculate the pH of a buffer solution prepared by dissolving 19.50 g of sodium cyanate NaCNO…

A: Mass of NaCNO = 19.50 g The number of moles of NaCNO, n = mass of NaCNO/molar mass of NaCNO…

Q: What [NH4CI] must be added to a solution of .154 M NH3 (aq) to make a buffer of pH 9.70? 0.342 O…

A: Buffer is solution which resist pH Change on addition on small amount of strong acid or strong base

Q: What is the pH of the solution after 40.5 mL of 0.200M NaOH has been added to 27.0mL of 0.300M HCI…

Q: Calculate the volume at which the pH= pKa if 30.00mL of weak acid with a concentration of 0.09885M…

A: Concentration of weak acid (M1) = 0.09885 M Volume of weak acid (V1) = 30.00 mL Concentration of…

Q: An analytical chemist is titrating 122.4 mL of a 0.2000M solution of propylamine (C,H,NH,) with a…

Q: Calculate the pH for each case in the titration of 50.0 mL of 0.120 M HCIO(aq) with 0.120 M KOH(aq).…

A: Note - Since you have asked a question with multiple subparts, we will do the first three subparts…

Q: A titration is performed in which 0.10 M LIOH is added to a 200.0 mL sample of 0.40 M HF. What is…

A: HF is a weak acid it reacts with LiOH which is a strong base and gives fluoride ion. Now this…

Q: A solution is made by adding 0.320 g Ca(OH)2(s), 35.0 mL of 1.10 M HNO3 and enough water to make a…

A: Given, Mass of Ca(OH)2 = 0.320 g Volume of HNO3 = 35.0 mL Molarity of HNO3 = 1.10 M Final volume…

Q: A 1.00 L buffer solution is 0.125 M in HF and 0.125 M in NaF. Calculate the pH of the solution after…

Q: You are given 250.0 mL of 0.100 M CH3CH2COOH (propionic acid, K, 1.35 x 10). Youd wish to adjust the…

A: pH is the proportion of hydrogen particle fixation in the solution. It is utilized to decide the…

Q: A titration is performed in which 0.14 M KOH is added to a 150.0 mL sample of 0.39 M HI. What is the…

A: PH of KOH can be calculated as follows

Q: 1. The pH of a buffer solution containing 0.5 mole/litre of CH:COOH and 0.5 mole/litre CH:COONA has…

Q: A chemist wishes to prepare a standard aqueous solution that has a concentration of Fe3+ equal to…

A: Please have a look into the solution:

Q: What is the pH value of a buffer solution prepared by dissolving 23.1 g of nahcoo salt in 0.432 M…

Question

A 25.0 mL sample of 0.200 M HCO2H(aq) is
titrated with 0.100 M KOH(aq). What is the
pH at the equivalence point? (Ka of HCO2H =
1.8 × 10-4)
8.28
O 8.52
O 7.00
O 10.26
5.71

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Introduction:

VIEW

Calculation:

VIEW

Result:

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps with 10 images

SEE SOLUTION Check out a sample Q&A here

Similar questions

A buffer is prepared in which the ratio [ H2PO4 ]/[ HPO42 ]is 3.0. (a) What is the pH of this buffer? (b) Enough strong acid is added to convert 15% of HPO42- to H2PO4-. What is the pH of the resulting solution? (c) Enough strong base is added to make the pH 7.00. What is the ratio of [H2PO4-] to [HPO42-] at this point?
You have a solution of the weak acid HA and add some of the salt NaA to it. What are the major species in the solution? What do you need to know to calculate the pH of the solution, and how would you use this information? How does the pH of the solution of just the HA compare with that of the final mixture? Explain.
Metacresol purple is an indicator that changes from yellow to purple at pH 8.2. (a) What is Ka for this indicator? (b) What is its pH range? (c) What is the color of a solution with pH 9.0 and a few drops of metacresol purple?
Ammonia gas is bubbled into 275 mL of water to make an aqueous solution of ammonia. To prepare a buffer with a pH of 9.56, 15.0 g of NH4Cl are added. How many liters of NH3; at 25C and 0.981 atm should be used to prepare the buffer? Assume no volume changes and ignore the vapor pressure of water.
What is an acidbase indicator? Define the equivalence (stoichiometric) point and the end point of a titration. Why should you choose an indicator so that the two points coincide? Do the pH values of the two points have to be within 0.01 pH unit of each other? Explain.
Calculate the pH of a buffer solution prepared from 0.155 mol of phosphoric acid, 0.250 mole of KH2PO4, and enough water to make 0.500 L of solution.
Sketch a titration curve for the titration of potassium hydroxide with HCl, both 0.100 M. Identify three regions in which a particular chemical species or system dominates the acid-base equilibria.
Blood contains several acid base systems that tend to keep its pH constant at about 7.4. One of the most important buffer systems involves carbonic acid and hydrogen carbonate ion. What must be the ratio of [HCO3] to [H2CO3] in the blood if the pH is 7.40?
What is the pH of the solution obtained by titrating 1.30 g of sodium hydrogen sulfate, NaHSO4, dissolved in 50.0 mL of water with 0.175 M sodium hydroxide until the equivalence point is reached? Assume that any volume change due to adding the sodium hydrogen sulfate or to mixing the solutions is negligible.
An important component of blood is the buffer combination of bicarbonate ion and carbonic acid. Consider blood with a pH of 7.42. a What is the ratio of [H2CO3] to [HCO3]? b What does the pH become if 15% of the bicarbonate ions are converted to carbonic acid? c What does the pH become if 25% of the carbonic acid molecules are converted to bicarbonate ions?
When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
A friend asks the following: Consider a buffered solution made up of the weak acid HA and its salt NaA. If a strong base like NaOH is added, the HA reacts with the OH to form A. Thus the amount of acid (HA) is decreased, and the amount of base (A) is increased. Analogously, adding HCI to the buffered solution forms more of the acid (HA) by reacting with the base (A). Thus how can we claim that a buffered solution resists changes in the pH of the solution? How would you explain buffering to this friend?