When the concentration of H+ ions in a solution decreases, a buffer maintains the pH of a solution by? It completely ionizes in solution to produce many H* ions.It partially ionizes in solution to produce few OH-ions.It partially ionizes in solution to produce few H+ ions.When the concentration of H+ ions in a solution decreases, a buffermaintains the pH of a solution byabsorbing H+ ionsreleasing H* ionsabsorbing OH-ionsreleasing OH- ionsSubmitThis form was created inside of WATERLOO REGION DISTRICT SCHOOL BOARD. Report ABGoogle FormsCleDELL

Introduction: A buffer is a weak acid or base that prevents sudden changes in the pH of the…

Answered: When the concentration of H+ ions in a…

Biomedical Instrumentation Systems

1st Edition

ISBN:9781133478294

Author:Chatterjee

Publisher:Chatterjee

Chapter19: Biomedical Laboratory Instrumentation

Section: Chapter Questions

Problem 7P

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Similar questions

When dissolved in water, a(n) _____ donates H+ and a(n) ______ accepts H+. a. acid; base b. base; acid c. buffer; solute d. base; buffer
Using a pH meter, you find the pH of an unknown solution to be 8.0. How would you describe this solution? a. weakly acidic b. strongly acidic c. weakly basic d. strongly basic
The pHpH scale for acidity is defined by pH=−log10[H+] where [H+]is the concentration of hydrogen ions measured in moles per liter (M). A solution has a pH of 10.2. Calculate the concentration of hydrogen ions in moles per liter (M).
Which of the following is a carbonic acid buffering molecule in a basic solution? Group of answer choices H2CO3 HCO3-
A buffer system .... a) All options are correct b) Counteracts pH changes in a solution c) Does the blood protein work as d) Releases protons (H +) if pH increases
The glass electrode used in commercial pH meters gives an electrical response proportional to the concentration of hydrogen ion. To convert these responses to a pH reading, the electrode must be calibrated against standard solutions of known H+ concentration. Determine the weight in grams of sodium dihydrogen phosphate (NaH2PO4 · H2O; FW 138) and disodium hydrogen phosphate (Na2HPO4 ; FW 142) needed to prepare 1 L of a standard buffer at pH 7.00 with a total phosphate concentration of 0.100 M . See Problem 24 for the pKa values of phosphoric acid.
A buffer donates OH- ions when conditions become too basic and accepts OH- ions when conditions become too acidic. is an acid that is used to offset overly basic conditions in the body. donates H+ ions when conditions become too basic and accepts H+ ions when conditions become too acidic. is a base that is used to offset overly acidic conditions in the body.
When two drops of NaOH were added to the water the color changed from purple to green. Did this make the pH: Increase stay the same decrease a lot decrease When HCI was added to water, the color changed from purple to hot pink. Did this make the pH: Increase stay the same decrease a lot decrease
Choose the FALSE statement An indicator can be used to monitor a buffer range When pH equals PKa of weak acid, the buffer capacity is the greatest Polyprotic acids have multiple stoichiometric points in their titration curve At the mid-point of titration of weak acid by strong base, the pH of the solution -does not equal the pKa of the weak acid The moles of titrant equals moles of titrate
Which of the following is most likely to be found evenly distributed in water in a homogeneous solution?a. sodium ions and chloride ionsb. NaCl moleculesc. salt crystalsd. red blood cells
In biological systems, buffers are important because they facilitate changes in pH to enhance biological activities of proteins and nucleic acids. True False
A small amount of NaOH is added to a weak acid buffer system. Describe what happens in terms of possible reactions and changes in pH.

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When the concentration of H+ ions in a solution decreases, a buffer maintains the pH of a solution by absorbing H+ ions releasing H* ions absorbing OH-ions releasing OH-ions