What is the pH of a solution that is 0.400M in formic acid and 1.00M in sodium formate?(Ka formic acid 1.80X 10-4)?Apply ( [H;O*]= Ka ( [Acid]/[conjugate base])( Ka = 1.08 X 10-4)НСООН + Н,0H3O*HCOO+НСО+ H,OНСООНOH+

Answered: Image /qna-images/answer/0cc4a484-1cab-449b-9a14-a83d527b6c3e.jpg

What is the pH of a solution that is 0.400M in formic acid and 1.00M in sodium formate? (Ka formic acid 1.80X 10-4)? Apply ( [H3O*]=Ka ( [Acid]/[conjugate base]) (Ka = 1.08 X 10-4) HCOOH + H,O H;O* HCOO НСОО + HО НСООН OH

What is the pH of a solution that is 0.400M in formic acid and 1.00M in sodium formate? (Ka formic acid 1.80X 10-4)? Apply ( [H3O]=Ka ( [Acid]/[conjugate base]) (Ka = 1.08 X 10-4) HCOOH + H,O H;O HCOO НСОО + HО НСООН OH

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.79QE

See similar textbooks

Related questions

Q: Calculate the ph of 1.55 M CH3NH2. The Kb for CH3NH2= 4.4 x 10^-4

Q: Part C. Classify whether the parameter shown in each item is describing an acidic or basic. Legend:…

Q: All weak bases have conjugate acids with Ka < 1.0 x 10-7 at 25 °C. True or False

Q: Conside following data on some weak acids and weak bases: acid base K. K, name formula name formula…

A: Whenver an acid and base reacts with each other than they form salt and water and the process is…

Q: Rank the compounds below in order of increasing acidity. " COH HO HO O2N Relevant Information: Kw=…

Q: Use the following table to predict the best acid / base pair for the desired pH/pOH value: pOH =…

Q: Calculate the pH at 25 °C of a 0.53M solution of pyridinium chloride (C5H,NHC1). Note that pyridine…

Q: Fourth Quarter GENERAL CHEMISTRY 2 Name: Strand, Gr. Level &Section: Date: ACTIVITY No. 3 -…

Q: A 0.25 M solution of a weak acid (HA) has a pH of 2.50. What is the Ka for this acid

Q: Which acid is stronger? Why? carbonic acid (Ka=4.2 x 10 -7) or formic acid (HCOOH, Ka=1.8 x…

Q: The pka of formaldehyde (H2C=0) is not listed in Table 6-1. (a) Based on your understanding of…

A: a.

Q: OUL UI 3 points. The boxes below contain a series of 0.1 M aqueous solutions of increasing pH where…

Q: Ka for formic acid (HCO2H) is 1.8 × 10^-4 . What is Kb for the formate ion (HCO2−)?

A: Answer: HCOOH (formic acid) is the weak organic acid and HCOO- (formate ion) is its conjugate base.

Q: a. [CH3 COOH] = 0.85 M, [CH;CO0-] = 0.45 M (the pK, for acetic acid is 4.74) pH = b. [Н,РО, ] 3 0.50…

Q: Show all steps: What is the percent ionization of a 1.38 mol/L weak base if its Kb = 2.7 x 10-6?

A: Given, concentration of weak base = 1.38 mol/L = 1.38 M Kb, = 2.7 x 10-6 % Ionization = ?

Q: At a temperature of 298K the value of Ka for ethanoic acid is 1.70 * 10Smoldm. c. Calculate the pH…

A: 1. Ka for ethanoic acid = 1.70 * 10-5 mol/dm3 = 1.70 * 10-5 M [ethanoic acid] = 0.350 mol/dm3 =…

Q: B: What is the pH of 0.6 M NHẠC1 solution? Discuss your results. (Kb of NH= 1.8 x 105) NH4* + H2O+…

A: In the given question we have to calculate the pH of 0.6 M NH4Cl Solution. we know that the ammonium…

Q: (Q19) What is the pH of a solution that is 0.720 in hydrosulfuric acid (H2S)? Ka1 = 8.9 x 10-8 and…

A: PH of H2S can be calculated as follows

Q: On acidity and basicity of aqueous solutions, the following relationships are valid, except…

Q: The Kb value for methylamine, CH3NH2, is 4.2 x 10-4. What is the pH of an aqueous solution for which…

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

Q: For 1-3. Calculate the pH, pOH and [OH-] of black coffee which is 5×10^-5 MH+ 20. 1. What is the…

A: The given data contains, H3O+=5×10-5M

Q: Part C. Classify whether the parameter shown in each item is describing an acidic or basic. Legend:…

A: For an acidic solution pH < 7 while for basic solution pH > 7 Since , pH + pOH = 14 So, for…

Q: 10. Given the pH of 1.5 M chloroacetic acid, CH2CICOOH solution is 1.96. a. Write an equation to…

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

Q: Calculate the ratio [CH3COOH]/[NaCH3COO] that gives a solution with pH = 5.00? Hint: Rearrange the…

Q: 13.Which of the following is the weakest acid? Group of answer choices H2SO4 HClO4 H3PO4 H4SiO4…

Q: 10. Given the pH of 1.5 M chloroacetic acid, CH2CICOOH solution is 1.96. a. Write an equation to…

A: The concept is that the stronger is the acid, weaker is its conjugate base.

Q: Calculate the pH at 25 °C of a 0.53M solution of ethylammonium bromide (C,H,NH,Br). Note that…

A: Given-> Concentration of C2H5NH3Br = 0.53 M pKb = 3.19

Q: Based on the data in the table below, which of the following is the strongest base? Organic Acid…

A: Sodium propionate has the strongest basicity.

Q: Methylamine, CH3NH2, has a Kb of 4.4 x 10-4. What is the pH of a 0.54 M solution of methylamine?…

Q: Calculate the pH at 25°C of a 0.58M solution of pyridinium chloride C5H5NHCl . Note that pyridine…

Q: Values of K, for Some Common Weak Bases Conjugate Acid Name Formula 1.8 × 10-5 4.38 × 10-4 5.6 ×…

A: Given: Kb of ammonia = 1.8×10-5

Q: Calculate the pH at 25 °C of a 0.44 M solution of lidocaine HCl (C¼H2 NONH,Cl). Note that lidocaine…

A: When pKb of a weak base is given, calculate 1) Kb value from pKb. 3) Calculate pOH from [OH-].…

Q: Calculate the pH of an aqueous solution that is 3.24 x 10-1 M oxopropanoic acid and 0.101 M sodium…

A: A buffer solution is a type of solution which can resist the pH change when small amount of acid or…

Q: At a temperature of 298K the value of Ka for ethanoic acid is 1.70 * 10$moldm3. c. Calculate the pH…

A: We will calculate both parts with the help of given information

Q: 1. a student prepares 0.1 M solution of formic acid(HCOOH) AND FOUND ITS ph at 25degrees to be 2.38.…

A: Consider the ionization of formic acid, HCOOH as below.The acid ionization constant, Ka of HCOOH is…

Q: What is the pH of a solution with [OH-]=2.2 x 10^-7M? Calculate the pH of a 0.0500M solution of…

Q: Given Methylamine (CH3NH2). Calculate pH of a 0.0010 M solution of this base. Given Kb for CH:NH2 is…

A: As per guidelines if multiple q uestions , first question is allowed to answer , please post…

Q: Would you help me whit this example (1) Thank you. ın a solutıon with a pH value of 7.0, Find…

A: Given : PH of solution = 7 Ka value of HOCl =3×10^-8 To find : percentage dissociation Solution :…

Q: I love you, Bartleby. Thank you for saving my life and career. I've learned so much!

Q: (a) Given that Ka for acetic acid is 1.8 x 10-5 and that forhypochlorous acid is 3.0 x 10-8, which…

A: (a) The Ka value for acetic acid (CH3COOH) is 1.8×10-5. The Ka value for hypochlorous acid (HOCl) is…

Q: Calculate the pH at 25 °C of a 0.54M solution of lidocaine HCl (C,„H¬NONH,CI). Note that lidocaine…

Q: If the Kb value for a weak base is 2.6*10^-4, what is the value of its conjugate acid?

Q: K, for benzoic acid, C6H; COOH, is 6.30 × 10-5. K, for phenol (a weak acid), C,H;OH, is 1.00 ×…

A: From the above data, Ka for acid is more = So, forming acid is the strongest acid. compared to…

Q: Use the following table to predict the best acid / base pair for the desired pH/pOH value: pH = 5.00…

A: Given : pH = 5.0 For acidic buffer : pH = pKa + log ( [conjugate base]/[acid]) For basic buffer: pOH…

Q: Calculate the pH at 25 °C of a 0.72M solution of lidocaine HCI (C4H2,NONH,CI). Note that lidocaine…

A: The value of pKb for the given weak base is = 7.94 The concentration of the base solution is = 0.72…

Q: What is the [H3O+] of 0.10 M propanoic acid (CH3CH2COOH, can simplify to HPr) (Ka= 1.3x10−5)?…

A: pH of a solution measures acidity of the solution. pH + pOH = 14 Where, pH = -log [H3 O+ ] and pOH…

Q: Formic acid (HCOOH) has a Ka = 1.8 × 10-4. What is the pH of a 25.00mL sample of 0.205 M formic…

A: Given: Ka = 1.8 × 10-4 [HCOOH] = 0.205 M

Q: Calculate the pH at 25 °C of a 0.47M solution of anilinium chloride (C,H;NH,CI). Note that aniline…

Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

What is the pH of a solution that is 0.400M in formic acid and 1.00M in sodium formate?
(Ka formic acid 1.80X 10-4)?
Apply ( [H;O*]= Ka ( [Acid]/[conjugate base])
( Ka = 1.08 X 10-4)
НСООН + Н,0
H3O*
HCOO
+
НСО
+ H,O
НСООН
OH
+

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

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 2 images

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

16-27 Guanidine, p/Ca 13.6, is a very strong base, almost as basic as hydroxide ion. NH NH2+ II II H2N—C—NH2 + H2O H2N—C—NH2 + OH" Guanidine Guanidinium ion pKb = 13.6 Complete the Lewis structure for guanidine, showing all valence electrons. The remarkable basicity of guanidine is attributed to the fact that the positive charge on the guanidinium ion is delocalized by resonance over the three nitrogen atoms. This delocalization increases the stability of the guanidinium ion relative to the ammonium ion or substituted ammonium ions. Draw three equivalent contributing structures for the guanidinium ion and show by the use of curved arrows how these three contributors are related. Propose an explanation for the fact that protonation occurs on the C=NH nitrogen rather than on one of the —NH., nitrogens. (Hint: Consider the resonance stabilization of the structure formed by protonation on a —NH., nitrogen compared with the resonance stabilization of the structure formed by protonation on the =NH nitrogen.) Predict the N—C—N bond angles in the hybrid. Which is the stronger acid, the ammonium ion or the guanidinium ion?
Use Table 13-3 to help answer the following questions. a. Which is the stronger base, ClO4 or C6H5NH2? b. Which is the stronger base, H2O or C6H5NH2? c. Which is the stronger base, OH or C6H5NH2? d. Which is the stronger base, C6H5NH2 or CH3NH2?
A 0.015M solution of a base has a pH of 10.09 a) What are the hydronium and hydroxide ion concentrations of this solution? b) Is the base a strong base, a moderately weak base (Ka of about 105) or a very weak base (Kb of about 1010)?
8-17 For each of the following, tell whether the base is strong or weak. (a) NaOH (b) Sodium acetate (c) KOH (d) Ammonia (e) Water
In calculating pH by ICE method of 0.015 M CH2FCOOH (Ka CH2FCOOH = 2.6 x10-3), the change in CH2FCOOH can not be neglected because. a. Acid Dissociation constant, Ka, has a negative exponent. b. pH is not within +/- pka unit of pka of CH2FCOOH c. initial CH2FCOOH concentration is less than 0.1 M d. dissociation of [CH2FCOOH] will be more than 5% of initial [CH2FCOOH] ----------- To protect corrosion of materials made of iron, the surface of the iron material is electroplated with another metal. Given below information, which metal will be best to “galvanize” the material ? O2 + H2O + 2e- -> 4OH-(aq) .... E0 = 0.401 v Fe2+(g) + 2e- - -> Fe ............ E0 =(-) 0.440 v Cu2+(g) + 2e- - -> Cu ...........E0 = 0.337 v Ni2+(g) + 2e- - -> Ni ............ E0 = (-)0.250 v Zn2+(g) + 2e- - -> Zn ............ E0 =(-) 0.763 v a. Zn b. Ni c. Cu d. Fe2+ ------------ Given : C (s) + H2O(g) <-> CO(g) + H2(g) Which of the following will shift equilibria to form…
Give typed explanation A 0.10 M solution of an acid, HA, has a pH of 3.0. What is the Kb of the conjugate base, A-, of this acid? For Kb, I got 9.1 x 10 ^-12. I want me make sure my answer is correct. Pleacse show steps and write clearly. Thank you!
5,Calculate the [OH-]of the solution with pH=10.50 Group of answer choices 1.05 x 10-10 5.0 x 10-10 3.2 x 10-10 3.2 x 10-4 6, Use the Ka values for the following acids to find the strongest conjugate base: HSO4- 1.2 x 10-2H2PO4- 6.3 x 10-8HCO3- 4.7 x 10-11 Group of answer choices A, H3PO4 B, H2SO4 C, HPO42- D, H2CO3 E, CO32- F, SO42-
Methylamine, CH3NH2, has a Kb of 4.4 x 10-4. What is the pH of a 0.54 M solution of methylamine? Your answer should be to two places past the decimal. Calculate the pH of a 0.21 M solution of hydrocyanic acid (HCN), which has a pKa of 9.31. Your answer should have 3 significant figures (i.e. 9.99).
Cyanic acid (HCNO) has Ka = 2.0 x 10-4 What is the conjugate base and its Kb value?
(a) Given that Ka for acetic acid is 1.8 x 10-5 and that forhypochlorous acid is 3.0 x 10-8, which is the stronger acid?(b) Which is the stronger base, the acetate ion or the hypochloriteion? (c) Calculate Kb values for CH3COO- and ClO-.
Would you help me whit this example (1) Thank you. ın a solutıon with a pH value of 7.0, Find the a1 and a0 values of hypchlorous acid ( For HOCl Ka=3x10^-8)
1. a student prepares 0.1 M solution of formic acid(HCOOH) AND FOUND ITS ph at 25degrees to be 2.38. calculate the Ka of formic acid. 2. 0.1 M FORMIC ACID CONTAINS 4.2 X10 ^-3,CALCULATE THE PERCENT TAGE OF h+ acid that is ionized