Compare the graphs of the known acidic solutions (HCl, HCOOH, H2SO4, and H3PO4). Which of these...
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Compare the graphs of the known acidic solutions (HCl, HCOOH, H2SO4, and H3PO4).
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Which of these acid(s) can act as a buffer and how was this determined?
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Which of these acid(s) cannot act as a buffer and how was this determined?
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Homework Answers
Buffer solution: Buffer solution is defined as the mixture of weak acid/weak base and its salt with strong base/strong acid.
Strong acid itself cannot act as a buffer, because it undergoes complete ionization and there is no equilibrium between undissociated and dissociated acid.
weak acids will develop equilibrium and they can act as Buffer solutions.
Acids which can act as buffer : HCOOH, H3PO4
Acids which cannot act as buffer : HCl, H2SO4
Add Answer to:
Compare the graphs of the known acidic solutions (HCl, HCOOH,
H2SO4, and H3PO4).
Which of these...
1 A) Which of the following pairs of solutions when mixed will form a buffer solution?...
1 A) Which of the following pairs of solutions when mixed will form a buffer solution? Group of answer choices H2SO4 and Ca(OH)2 NH3 and NH4Br NaNO3 and HNO3 KOH and KNO2 B)Phosphoric acid, H3PO4, is a triprotic acid with the following Ka values: Ka1 = 7.5 x 10-3; Ka2 = 6.2 x 10-8; Ka3 = 3.6 x 10-13 In a solution of 0.15 M H3PO4, which species will be most abundant? H3O+ H3PO4 HPO42- H2PO4-
1) Which compound would be more soluble in an acidic solution than in a neutral solution?...
1) Which compound would be more soluble in an acidic solution than in a neutral solution? A. AgCl B. CuBr2 C. SrF2 D. PbI2 2) A buffer solution is composed of 0.200M NH3 and 0.200 M NH4Cl. When a small amount of HCl is added to this buffer, which species in the buffer neutralizes the added acid? A. ammonium ion, NH4+ B. chloride ion, Cl- C. ammonia, NH3 D. None of the above since HCl cannot be neutralized by this...
Calculate the pH and pOH of the following solutions: a. stomach acid in which [HCl] =...
Calculate the pH and pOH of the following solutions: a. stomach acid in which [HCl] = 0.155 M b. 0.00500 M HNO3 c. a 2:1 mixture of 0.0125 M HCl and 0.0125 M NaOH d. a 3:1 mixture of 0.0125 M H2SO4 and 0.0125 M KOH
To have solutions of HCl and acetic acid (CH3CO2H) with the same pH, which of the...
To have solutions of HCl and acetic acid (CH3CO2H) with the same pH, which of the following needs to be done? The concentration of each solution needs to be the same. The concentration of HCl needs to be higher. The concentration of acetic acid needs to be higher. The solutions can never have the same pH. Volume of acetic acid solution must be lower.
Question 5 1 pts A student mixes HCl and NaCl (source of conjugate) and claims to...
Question 5 1 pts A student mixes HCl and NaCl (source of conjugate) and claims to have made a buffer. Is this claim accurate? Yes- it is a mixture of acid and conjugate base after all Yes- any acid with a conjugate can make a buffer Oo oo C No-the conjugate base is so weak it does not reach equilibrium with water Need more information Question 6 1 pts Which combination of acid and base would create a buffer? Assume...
Which of the following sets of chemicals can be used to prepare buffer solutions? For each...
Which of the following sets of chemicals can be used to prepare buffer solutions? For each one that can, identify the weak acid and its conjugate base. Include charge (if any) and phase. Enter "none" for both if a buffer is not possible. A.) Na2HPO4+HCl Is a buffer possible (Yes or No) and what is the weak acid and what is the conjugate base B.)NH4Cl+NH3 Is a buffer possible (Yes or No) and what is the weak acid and conjugate...
This is from a Study of Buffer Solutions and pH of Salt Solutions Lab. I calculated...
This is from a Study of Buffer Solutions and pH of Salt
Solutions Lab. I calculated Ka to be 3.2*10^-5. Why is my value
larger than the standard value?
Procedure:
10. How does your calculated value of Ka compare with the standard value of Ka for acetic acid? Discuss why your value may be larger or smaller than the standard value. Caleutats Ka 3.2x 10-5) Cyato-s Learning Objectives: 1. To test the acidic and basic properties of ionic compounds 2....
unknown solutions A and B are 0.1 M solutions of either HCI or NaOH. According to your pH measurement, which is which...
unknown solutions A and B are 0.1 M solutions of
either HCI or NaOH. According to your pH measurement, which is
which
10% Bleach Question: 1. Unknown solutions A and B are 0.1 M solutions of either HCl or NaOH. According to your pH measurements, which is which? 1 2. The pH of pure water is 7. Comment on how closely your measured pH values from each measurement method compared to the expected value. Which method was more appropriate for...
In this lab, we will observe how weak acid solutions can work as a buffer. In...
In this lab, we will observe how weak acid solutions can work as a buffer. In this context, "buffer" refers to a solution that maintains a nearly constant pH, which is essential for biological systems to function properly. For example, the pH of human blood varies only slightly between the values of 7.35-7.45. Which of the following statements is true regarding the "buffer" in this context? "Buffer" refers to any solution that contains acid and base. All buffers can maintain...
A) Which of the following pairs cannot be mixed together to form a buffer solution? Why?...
A) Which of the following pairs cannot be mixed together to form a buffer solution? Why? A. NH3, NH4Cl B. KOH, HF C. NaC2H3O2, HCl D. H3PO4, KH2PO4 E. RbOH, HCl I already know the answer is E. I want help understanding when we can rule out choices B and C. B) For a solution equimolar in HCN and NaCN, which statement is false? Without giving all the choices, the false choice is "The [H+] is larger than it would...
Question 5 1 pts A student mixes HCl and NaCl (source of conjugate) and claims to have made a buffer. Is this claim accurate? Yes- it is a mixture of acid and conjugate base after all Yes- any acid with a conjugate can make a buffer Oo oo C No-the conjugate base is so weak it does not reach equilibrium with water Need more information Question 6 1 pts Which combination of acid and base would create a buffer? Assume...
This is from a Study of Buffer Solutions and pH of Salt
Solutions Lab. I calculated Ka to be 3.2*10^-5. Why is my value
larger than the standard value?
Procedure:
10. How does your calculated value of Ka compare with the standard value of Ka for acetic acid? Discuss why your value may be larger or smaller than the standard value. Caleutats Ka 3.2x 10-5) Cyato-s Learning Objectives: 1. To test the acidic and basic properties of ionic compounds 2....
unknown solutions A and B are 0.1 M solutions of
either HCI or NaOH. According to your pH measurement, which is
which
10% Bleach Question: 1. Unknown solutions A and B are 0.1 M solutions of either HCl or NaOH. According to your pH measurements, which is which? 1 2. The pH of pure water is 7. Comment on how closely your measured pH values from each measurement method compared to the expected value. Which method was more appropriate for...
In this lab, we will observe how weak acid solutions can work as a buffer. In this context, "buffer" refers to a solution that maintains a nearly constant pH, which is essential for biological systems to function properly. For example, the pH of human blood varies only slightly between the values of 7.35-7.45. Which of the following statements is true regarding the "buffer" in this context? "Buffer" refers to any solution that contains acid and base. All buffers can maintain...
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