(a)
Interpretation:
The pH of the 0.1 M HCl solution needs to be calculated.
Concept introduction:
The pH of the solution is defined as negative log of hydrogen ion concentration in the solution.
It is mathematically represented as follows:
Here,
(b)
Interpretation:
The pH of 0.1 M NaOH needs to be calculated.
Concept introduction:
The pH of the solution is defined as negative log of hydrogen ion concentration in the solution.
It is mathematically represented as follows:
Here,
(c)
Interpretation:
The pH of 0.05 M HCl solution needs to be calculated.
Concept introduction:
The pH of the solution is defined as negative log of hydrogen ion concentration in the solution.
It is mathematically represented as follows:
Here,
(d)
Interpretation:
The pH of 0.05 M NaOH needs to be calculated.
Concept introduction:
The pH of the solution is defined as negative log of hydrogen ion concentration in the solution.
It is mathematically represented as follows:
Here,
Want to see the full answer?
Check out a sample textbook solutionChapter 1 Solutions
Biochemistry
- The-carotene molecule has λmax 450 nm and ɛ = 15.000 m2 / mol. Calculate the expected absorbance value for a solution in which 0.1 mg is dissolved in 10 mL of water. ( β-carotene, C40H56, 536 g/mol path length 1 cm)arrow_forwardSoft drinks usually have a pH of approximately 3.1. What is the [H3O+] concentration in a soft drink?arrow_forwardEnter be balanced equation for the ionization of butanoic acid, carboxylic acid, in water. Express your answer as a chemical equation without phases.arrow_forward
- Alligation Alternate. Show your complete solution. Note: Indicate the unit. Indicate your answer in whole numbers. 1. The solvent for the extraction of a vegetable drug is 75% alcohol. How many milliliters may 95%, 60% and 50% alcohol be mixed to prepare 75% of 4 pints of alcohol? Amount of 95% alcohol needed = ? Amount of 60% alcohol needed = ? Amount of 50% alcohol needed = ?arrow_forwardans fast I will upvote A sample of PbSO4 solid has reached equilibrium in a beaker of water. If the ionic strength of the solution is then increased by adding LINO3 salt what happens to the activity coefficients of the Pb+2 and what happens to the solubility of the PbSO4 choose the option and explain the activity coefficient will increase and the molar solubility will decrease Both activity coefficient the molar solubility will decrease the activity coefficient will decrease and the molar solubility will increase Both activity coefficient the molar solubility will increasearrow_forwardTONICITY The salinity (concentratin of NaCl) if human blood is 0.9%. Imagine an evil nurse injected a 15% saline solution into a poor patient. What do you predict will happen to the patient's red blood cells? Answer in the textbox provided below.arrow_forward
- Disadvantages of cholesterolarrow_forwardAt a pH of 7.40, the carbonic acid ratio is ________. a. 35:1 b. 4:1 c. 20:1 d. 3:1arrow_forwardMATHEMATICAL A catalog in the lab has a recipe for preparing 1 L of a TRIS buffer at 0.0500 M and with pH 8.0: dissolve 2.02 g of TRIS (free base, MW=121.1 g/mol) and 5.25 g of TRIS hydrochloride (the acidic form, MW=157.6 g/mol) in a total volume of 1 L. Verify that this recipe is correct.arrow_forward
- Cellular pH is slightly alkaline (pH 7.4); Explain why a seemingly slight decrease in pH to 6.8 can have very serious consequences for the body, becoming fatal?arrow_forwardConsider a buffer solution that contains 0.55 M NH2CH2CO2H and 0.35 M NH2CH2CO2Na. pKa(NH2CH2CO2H)=9.88. a. Calculate its pH. b. Calculate the change in pH if 0.155 g of solid NaOH is added to 250 mL of this solution. c. If the acceptable buffer range of the solution is ±0.10 pH units, calculate how many moles of H3O+ can be neutralized by 250 mL of the initial buffer.arrow_forwardYou need a buff er at pH 7.5 for use in purifying a protein at 4°C. You have chosen Tris, pK 8.08, ΔH° = 50 kJ · mol−1. You carefully make up 0.01 M Tris buffer, pH 7.5 at 25°C, and store it in the cold to equilibrate it to the temperature of the purifi cation. When you measure the pH of the temperature-equilibrated buff er it has increased to 8.1. What is the explanation for this increase? How can you avoid this problem?arrow_forward
- Anatomy & PhysiologyBiologyISBN:9781938168130Author:Kelly A. Young, James A. Wise, Peter DeSaix, Dean H. Kruse, Brandon Poe, Eddie Johnson, Jody E. Johnson, Oksana Korol, J. Gordon Betts, Mark WomblePublisher:OpenStax CollegeEssentials of Pharmacology for Health ProfessionsNursingISBN:9781305441620Author:WOODROWPublisher:Cengage
- BiochemistryBiochemistryISBN:9781305961135Author:Mary K. Campbell, Shawn O. Farrell, Owen M. McDougalPublisher:Cengage Learning