2. a. What is the ratio of H2PO4 to H3PO4 at a pH of3? Phosphoric acid, pKal =2.12, pKa2 = 7.21, and pKa3 12.32 %3D %3D b. If 3 volumes of 9 mM NaOH are mixed with 1 volume of 20 mM Phosphoric acid (H3PO4), what will be the pH of the final mixture?

2. a. What is the ratio of H2PO4 to H3PO4 at a pH of3? Phosphoric acid, pKal =2.12, pKa2 = 7.21, and pKa3 12.32 %3D %3D b. If 3 volumes of 9 mM NaOH are mixed with 1 volume of 20 mM Phosphoric acid (H3PO4), what will be the pH of the final mixture?

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 7ALQ: You have a solution of the weak acid HA and add some HCl to it. What are the major species in the...

See similar textbooks

Related questions

Q: What is the pH of a solution that contains 0.12 M HC2H3O2 and 0.29 M C2H3O2? Use Kb = 5.6 x 10-10…

Q: Suppose you are given solutions of 1.00 M acetic acid and 1.00 M sodium acetate and are asked to…

A: This is a buffer solution so pH = pKa + log ([salt]/[Acid])

Q: uppose a solution of NaOH was titrated and found to have a molarity of 0.250 M. This solution is now…

Q: What volume of 0.120 M NaOH must be added to 100 mL of 0.100 M NaHC204 to reach a pH of 4.70? H2C204…

A: The solution is given below -

Q: A 0.128 g sample of KHP (HKC8H4O4) required 28.54 mL of NaOH solution to reach a phenolphthalein…

A: Solution:- Given data = 0.128 g of KHP (HKC8H404) Volume of NaOH used = 28.54 mL = 0.02854 L Molar…

Q: What is the final pH of a solution obtained by mixing 450 ml of 0.20 M NaOH with 150 ml of 0.10 M…

A: H3PO4 is a tri-protic acid ( it have 3 acidic Protons ) , so when NaOH is added to it, protons would…

Q: What is the pH of a solution of 0.300 M HNO₂ containing 0.100 M NaNO₂? (Ka of HNO₂ is 4.5 × 10⁻⁴)

A: Ka = 4.5*10^-4 (given) pKa = – log [ Ka ] = – log(4.5*10^-4) = 3.347 Now, By using Henderson…

Q: 4. Tris(hydroxymethyl)aminomethane [(HOCH2)3CNH2–Tris, or THAM] is a weak base frequently used to…

A: Buffers are the mixtures that resists change in pH when small amount of acid or base is added to it.…

Q: 2. The active component of aspirin is acetylsalicylic acid, HC,H,0, which has a Ka of 3.0 x 10-4.…

A: Answer: In this question a weak organic acid acetylsalicylic acid is given to us and we have…

Q: 5- Instrumental methods of analysis example such 6- Acid equivalent weight can calculated by…

A: Fill in the blanks are given as:

Q: 3) i) A 25.0mL sample of a 30.0% HF solution has a density of 1.101g/mL. The sample is diluted to a…

A: (i) Given, Initial volume of the solution is 25.0 mL. Final volume of the solution is 500 mL.…

Q: The chief chemist of Victory Vinegar Works, Ltd., inter- views two chemists for employment. He…

A: The reaction of acid and base in the presence of an indicator in the laboratory is called titration.…

Q: hat mass of Ca(OH)2 is present in 125.00 ml of Ca(OH)2(aq) solution that has pH = 12.15?

Q: ) How many moles of BHCl (acidic salt) would need to be added to 452 mL of 1.66 M B (a weak base) to…

A: The question is based on the concept of buffer solution. A buffer is a solution which resist any…

Q: What is the pH of a solution of 0.400 M CH₃NH₂ containing 0.250 M CH₃NH₃I? (Kb of CH₃NH₂ is

A: The question is based on the concept of PH calculations. we have to apply henderson equation to…

Q: What is the pH of 500 mL of water after the addition of 1 mL of 2M NaOH? HINT: you cannot use H-H…

A: A solution that resist any change in the pH is called a buffer solution. The pH of a buffer solution…

Q: 1. Complete the reaction Mg(OH)2 Mg+2 +2 ionization 2. What is the pH of a 0.001000 M Mg(OH)2…

A: The reaction given is, =>

Q: What volumes of stock 0.500 M sodium propanoate and 0.500 M propanoic acid (pKa 4.88) are needed to…

Q: Anilinium chloride (C6H5NH3Cl) is a weak acid (Ka = 2.4 x 10-5). A sample of anilinium chloride…

A: “Since you have posted a question with multiple sub-parts, we will solve first three subparts for…

Q: What is the volume of HF (ideal gas at 1 atm and 25°C) required to be bubbled into 250 ml distilled…

A: pH = 2.50 -log (H)+ =2.50 H+=10-pH=10-2.50=0.00316 M

Q: A diprotic weak base (B) has pK, values of 4.058 (pK) and 7.102 (pKa). Calculate the fraction of the…

Q: What is the resulting pH of mixing 50.0 ml 0.0500 M NH4Cl (aq) with 10.0 ml 0.0500 M HNO3(aq)? If…

A: Given : Molar concentration of NH4Cl = 0.0500 M Volume of NH4Cl solution = 50.0 ml Molar…

Q: A diprotic weak base (B) has pKp values of 3.510 (pKp1) and 6.143 (pKp2). Calculate the fraction of…

A: Given data: pKb1 = 3.510 pKb2 = 6.143 pH = 9.429 Formula used: pKa = 14 - pKb pKa = -log [Ka] pH…

Q: Trial 1 Initial Burette 1ml Reading (mL) Endpoint (mL) 11.75 Endpoint (pH) 12.91 10.56 Equivalence…

A: In this question we have to calculate the theoretical molarity and actual molarity from the given…

Q: Question: pH pf 50.0 mL H20 + 1.00 mL 0.6 M HCl (below is the data to answer the answer)…

A: Formula pH = -log [H+] Molarity = Moles of soluteL of solution Moles = Molarity x L of solution

Q: 3.Tris(hydroxymethyl)aminomethane [(HOCH2)3CNH2-Tris or THAM] is a weak base frequently used to…

A: Given: Kb=1.2×10-6pKb= 5.92pKa=8.08 Volume of HCl= 100mL Concentration of HCl= 0.50M pH of buffer=…

Q: Why is [ H3O]=[OH-]=1.0× ^ -2 not feasible in water? What would happen if we tried to make such a…

A: Since the water has an equilibrium with H3O+ and OH- ions as per the reaction 2 H2O (l)…

Q: What is the pH of 0.15 M acetic acid to 1.00 L of which 2.70 g of sodium acetate NaCH3CO2, has been…

A: Given: Molarity of acid = 0.15 M Volume of sodium acetate = 1.00 L Mass of sodium acetate = 2.70 g…

Q: 2. The active component of aspirin is acetylsalicylic acid, HC,H,0., which has a K. of 3.0 x 10-4…

A: 2) Given: Ka of HC9C7O4 = 2.0 × 10-4 a) Given: Mass of HC9C7O4 = 0.500 g. And volume of solution =…

Q: Aspirin was discovered as a result of efforts to produce a derivative of salicylic acid that would…

A: The pH of a solution of Aspirin (acetylsalicylic acid) with the concentration of 2.502M is to be…

Q: Solve this?

A: pH = 9.2 pH + pOH = 14 pOH = 14-9.2 = 4.8

Q: Propanoic acid (CH3CH2COOH) has a Ka of 1.3×10–5. FW(propanoic acid) = 74.08 g/mol; FW(calcium…

A: Buffers are generally good over the range pH = pKa ± 1. For example, the acetate buffer would be…

Q: 3. Complete neutralization of 10 ml. of phosphoric acid solution by NaOH 0.I N in the presence of…

A: During titration of phosphoric acid we can use either methyl orange and detect first end point…

Q: CICH2 CO2 H HNO C2H2CINA O 1.80mol of monochloroacetic acid 0.80 mol of Nitric acid, 0.80 mol of…

Q: What is the pH at 25°C of a solution that results from mixing equal volumes of a 0.0500 M solution…

A: The pH of a solution is related to the acid dissociation constant by the Henderson-Hasselbalch…

Q: The Kb of HONH2 is 1.1x10^-8 a. calculate the pH and percent dissociation of a solution…

Q: How many milliliters (mL) of 5.0 M HCl should be added to 26.6 g of sodium borate to give a pH of…

A: Boric acid(HA) is a weak acid and sodium borate(A-) is a conjugate base of boric acid. Hence they…

Q: Phenylacetic acid (C6H5CH2CO2H) is a weak monoprotic acid with Ka=4.90x10-5. what is the pH that…

A: Here we are required to find the pH of the solution

Q: Calculate the pH of 5.40 g of K2SO3 that has been completed with 500 mL H2O (pKa1= 1.85 and pKa2 =…

A: Weight of K2SO3 = 5.4 g Mol mass of K2SO3 = 158.26 g/mol Volume of H20 = 500 ml Calculation is done…

Q: A natural water is in equilibrium with CO2 and CaCO3. Calculate pH if the mixing ratio of CO2 is 620…

A: Answer - The correct option is (c) - 8.45

Q: FRQ1: Consider the titration of 25.00 ml of 0.08 M of a weak acid, HA, with 0.125 M NAOH. Calculate…

A: We are authorized to answer three subparts at a time, since you have not mentioned which part you…

Q: Bar Keepers Friend is a household cleaner containing oxalic acid, a diprotic acid where pKa1 = 1.27…

A: PKa1 and PKa2 values are given as 1.21 and 4.27 respectively. Hence, it is possible to determine the…

Q: A reaction was carried out between 18 ml of a 0.05 M solution of hydrochloric acid with 24 ml of a…

Q: Calculate how many milliliters of 0.140 M HNO3 should be added to 200 mL containing 2.00 g K2CO3…

A: Here we have to determine the volume in ml of HNO3 solution of 0.140M to be added to 200ml of so2 g…

Q: 17.18

Q: Pure water is neutral in pH or has a pH value of exactly 7.00. How does the pH of pure water vary…

A: Pure water has a neutral pH of 7. When water undergoes the distillation process or when it is…

Q: A sample is known to contain NaOH (MM 40.02), Na₂CO3 (MM 105.79), NaHCO, (MM 84.01) or a compatible…

Q: = H+ + HPO;- Ka = 6.2 x 10-8 = H+ + SO?- Ka = 1.3 x 10-2 From the systems above, identify the…

A: The question is based on the concept of buffer solution. A buffer is a solution which resist any…

Q: What would be the pH of a 100mL solution containing 0.24M formic acid (HCHO2; Ka= 1.8x10 -4) and…

A: Formic acid (a weak acid) and sodium formate (Salt of formic acid with NaOH) forms an acidic buffer…

Question

2. a. What is the ratio of H2PO4 to H3PO4 at a pH of3?
Phosphoric acid, pKal 2.12, pKa2 = 7.21, and pKa3 = 12.32
%3D
%3D
b. If 3 volumes of 9 mM NaOH are mixed with 1 volume of 20 mM
Phosphoric acid (H3PO4), what will be the pH of the final mixture?

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

Step 1

Step 2

Step 3

Step 4

Trending now

This is a popular solution!

Step by step

Solved in 4 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Weak base B has a pKb of 6.78 and weak acid HA has a pKa of 5.12. a Which is the stronger base, B or A? b Which is the stronger acid, HA or BH+? c Consider the following reaction: B(aq)+HA(aq)BH+(aq)+A(aq) Based on the information about the acid/base strengths for the species in this reaction, is this reaction favored to proceed more to the right or more to the left? Why? d An aqueous solution is made in which the concentration of weak base B is one half the concentration of its acidic salt, BHCl, where BH+ is the conjugate weak add of B. Calculate the pH of the solution. e An aqueous solution is made in which the concentration of weak acid HA twice the concentration of the sodium salt of the weak acid, NaA. Calculate the pH of the solution. f Assume the conjugate pairs B/BH+ and HA/A are capable of being used as color-based end point indicators in acidbase titrations, where B is the base form indicator and BH is the acid form indicator, and HA is the acid form indicator and A is the base form indicator. Select the indicator pair that would be best to use in each of the following titrations: (1) Titration of a strong acid with a strong base. (i) B/BH+ (ii) HA/A (2) Titration of a weak base with a strong acid. (i) B/BH+ (ii) HA/A
Amino acids are an important group of compounds. At low pH, both the carboxylic acid group (CO2H) and the amine group (NHR) are protonated. However, as the pH of the solution increases (say, by adding base), the carboxylic acid proton is removed, usually at a pH between 2 and 3. In a middle range of pHs, therefore, the amine group is protonated, but the carboxylic acid group has lost the proton. (This is called a zwitterion.) At more basic pH values, the amine proton is dissociated. What is the pH of a 0.20 M solution of alanine hydrochloride, [NH3CHCH3CO2H]Cl?
What are the major species in solution after NaHSO4 is dissolved in water? What happens to the pH of the solution as more NaHSO4 is added? Why? Would the results vary if baking soda (NaHCO3) were used instead?
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.
The simplest amino acid is glycine, H2NCH2CO2H. The common feature of amino acids is that they contain the functional groups: an amine group, -NH2, and a carboxylic acid group, -CO2H. An amino acid can function as either an acid or a base. For glycine, the acid strength of the carboxyl group is about the same as that of acetic acid. CH3CO2H, and the base strength of the amino group is slightly greater than that of ammonia, NH3. (a) Write the Lewis structures of the ions that form when glycine is dissolved in 1 M HCl and in 1 M KOH. (b) Write the Lewis structure of glycine when this amino acid is dissolved in water. (Hint: Consider the relative base strengths of the -NH2 and -CO2- groups.)
In dilute aqueous solution HF acts as a weak acid. However, pure liquid HF (boiling point = 19.5 C) is a strong acid. In liquid HF, HNO3 acts like a base and accepts protons. The acidity of liquid HF can be increased by adding one of several inorganic fluorides that ale Lewis acids and accept F- ion (for example, BF3 or SbF5]. Write balanced chemical equations for the reaction of pure HNO3 with pure HF and of pure HF with BF3.
Isocyanic acid (HNCO) can be prepared by heating sodium cyanate in the presence of solid oxalic acid according to the equation 2NaOCN(s)+H2C2O4(s)2HNCO(l)+Na2C2O4(s) Upon isolating pure HNCO(l), an aqueous solution of HNCO can be prepared by dissolving the liquid HNCO in water. What is the pH of a l00.-mL solution of HNCO prepared from the reaction of 10.0 g each of NaOCN and H2C2O4, assuming all of the HNCO produced is dissolved in solution? (Ka of HNCO = 1.2 l04.)
The hydrogen phthalate ion, C8HsO4, is a weak acid with Ka = 3.91 106. C8H5O4(aq)+H2O(l)C8H4O42(aq)+H3O+(aq) What is the pH of a 0.050 M solution of potassium hydrogen phthalate. KC8H5O4? Note: To find the pH for a solution of the anion, we must take into account that the ion is amphiprotic. It can be shown that, for most cases of amphiprotic ions, the H3O+ concentration is [H3O+]=Ka1Ka2 For phthalic acid, C8H6O4 is Ka1 is 1.12 103, and Ka2 is 3.91 106.
Phenol, C6H5OH, is a weak organic acid. Suppose 0.515 g of the compound is dissolved in enough water to make 125 mL of solution. The resulting solution is titrated with 0.123 M NaOH. C6H5OH(aq) + OH(aq) C6H5O(aq) + H2O() (a) What is the pH of the original solution of phenol? (b) What are the concentrations of all of the following ions at the equivalence point: Na+, H3O+, OH, and C6H5O? (c) What is the pH of the solution at the equivalence point?
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?
The pH of a solution of Ba(OH)2 is 10.66 at 25 . What is the hydroxide ion concentration in the solution? If the solution volume is 125 mL, what mass of Ba(OH)2 must have been dissolved?
Does the pH of the solution increase, decrease, or stay the same when you (a) Add solid sodium oxalate, Na2C2O4, to 50.0 mL of 0.015-M oxalic acid? (b) Add solid ammonium chloride to 100. mL of 0.016-M HCl? (c) Add 20.0 g NaCl to 1.0 L of 0.012-M sodium acetate, NaCH3COO?