Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 10: Q16P (page 231)

Phosphate at0.01Mis one of the main buffers in blood plasma, whose pH is 7.45. Would phosphate be as useful if the plasma pH were 8.5?

Short Answer

Expert verified

As a result, at pH=8.50, phosphoric acid would be less beneficial.

Step by step solution

01

Definition of Phosphoric acid

  • Phosphoric acid (H3PO4), also known as orthophosphoric acid, is the most important oxygen acid of phosphorus and is used to generate fertiliser phosphate salts.
  • It's also employed in dental cements, albumin derivative manufacturing, and the sugar and textile sectors.
02

Determine the phosphate is useful if the plasma pH were 8.5

  • Phosphate with 0.01MOne of the buffers in blood plasma is concentration. It look at if the phosphate would be as effective if the plasma pH was 8.50.
  • Search at the Pg899 and look in the Table for the phosphoric acid's pKawhich is pK_{a}=7.198.
  • #c34632the amount of moles of a base or an acid required to adjust the pH of a solution by one is known as buffer capacity.
  • At pH=7.45, phosphoric acid has a high buffer capacity, while at pH=8.50, it has a low buffer capacity.
  • As a result, at pH=8.50, phosphoric acid would be less beneficial.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

How many millilitres of 1.00 M KOH should be added to 100 mL of solution containing 10.0 g of histidine hydrochloride

[His? HCI (HisH1) (CI2), FM 191.62 ] to get a pH of 9.30 ?

Find the pH with 1.50gNaN2Pinstead of 1.20 g.

Draw the structures of the predominant forms of glutamic acid and tyrosine at pH9.0and pH10.0What is the second most abundant species at each ?.

The acid HA has pKa=7.00.

(a) Which is the principal species, HA or A-, at pH 6.00?

(b) Which is the principal species at pH 8.00?

(c) What is the quotient [A-]/[HA] at pH 7.00? At pH 6.00?

(a) Copy column B of your spreadsheet and paste it into columnG. ChangeK1to10-4in cell G5 and change K2 to 10-8 in cell G6. Change F to 0.01 in cell G8. Column G now contains concentrations for the amphiprotic salt Na+HA-withK1=10-4,K2=10-8, andF=0.01M. Check the answers by hand beginning with pH=12(pK1+pK2). With[HA-],F, calculate[H2A]and[A2-]. Then find[HA-]>>F-[H2A]-[A2-].

(b) Copy column G of your spreadsheet and paste it into column H. Change K2 to 10-5 in cell G6. Column G now contains the concentrations for the intermediate form of a diprotic acid with K1=10-4, K2=10-5, and F =0.01M. You should observe[HA-]=6.13×10-3Mand pH=4.50.
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Analysis

Read Explanation

Nuclear Chemistry

Read Explanation

Kinetics

Read Explanation

Chemistry Branches

Read Explanation

The Earths Atmosphere

Read Explanation

Ionic and Molecular Compounds

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free