2. A solution of pH 12 will contain a large concentration of(fill in)a. Cl-b. Na+С. ОН-d. H+ions. Buffers are substances that keep the pH of a solution stable. In blood, the mainbuffer system is carbonic acid-bicarbonate in which bicarbonate acts as thea. H+ suppressorb. H+ асceptorc. H+ donord. H+ processorH,CO3HCO,-+Looking at the above equation we can deduct that if an acidic solution is injected in theblood of a person, the above equilibrium will move to thea. rightb. leftThe action of buffers in the blood is important to keep the pH stable aroundа. 7.4b.7.0с. 7.8d. 6.8In the human stomach, digestive enzymes require a high concentration ofa. hydroxide ionsb. protonsc. cholesterold.inositolfor optimal function.

"Since there are multiple questions and it is not mentioned that which one has to be solved so I am solving only the first part. Please repost the other questions if you need answers for them too." The pH of a particular substance is the negative logarithm of the (H+) hydrogen ion concentration. It can have values from zero to fourteen. The pH value of less than 7 specifies that the substance is an acid, the pH value of more than 7 specifies that the substance is a base and the pH of 7 specifies a neutral compound.The solution with pH value of 12 is basic in nature. A basic solution always contains more hydroxide ion (OH-) concentration than hydrogen ion (H+) concentration. Thus, the solution of pH 12 contains large OH- concentration. Answer: Option c (OH-) is correct.

Answered: 2. A solution of pH 12 will contain a…

Science

Chemistry

2. A solution of pH 12 will contain a large concentration of (fill in) а. C- b. Na+ с. ОН- d. H+

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Indicate if the following solutions are acidic or basic. Consider 25 °C. а. рH%3D2.50 b. [H*]> 1.0 x 10-7 с. РОН 3D 3.28 d. [OH]= 2.11 × 10-12 M
5. Determine the pH of the solution which has 10% of NaOH in deionized water by mass. The NaOH which was used to prepare 10% solution has a density of 1.131kg/L. Assumption: 100 % dissociation. N2OH + Na* + OH
In the process, H2O + CN- → HCN + OH- , ______ acts a Bronsted-Lowry base. A. H2OB. CN- C. HCND. H3O+E. OH
The pH of a 0.92M solution of hypobromous acid (HBRO) is measured to be 4.34. Calculate the acid dissociation constant K, of hypobromous acid. Round your answer to 2 significant digits. K %3D a x10 Canti 2021 McGraw Hill LLC.
A solution was found to have a pOH of 13.11 at 25 °C. What is the concentration of Ht? а. О.13 М b. 7.8 x 10-28 M c. 0.89 M d. 0.05 M e. 7.8 x 10-14 M
4. Calculate [H,O*], [OH ], pH, and pOH for 6.5 x 10³ M H₂SO, solution (at 25 °C). a. [H,0¹] b. [OH] c. pH d. pOH
b. I'm falling asleep.... The CO₂ concentration in a classroom can increase over the lecture period due to poor ventilation. You decide to measure the pH of pure water in contact with the atmosphere as an indirect way to determine whether you have adequate ventilation. You measure a pH value of 5.3. Assuming equilibrium, i. What is the concentration of CO2 in the classroom? ii. How does the value you calculated compare to the recommended safe level of 800-1000 ppm?
Answers with solu
15. Dimethylamine (CH3)2NH is a weak base with a pKą of 11.0 Calculate the pH of a solution of dimethylamine at 0.40 mol.L-1. b. Calculate the pH of a solution of dimethylamine at 4.0 x 10-2 mol.L-¹.
Succinic acid is a diprotic acid with pka1=4.21 and pKa2=5.63. The three forms (abbreviated H₂A, HA¯, and A²-) are shown below. Consider a 0.10 M H₂A solutions. HO. HO. a. Rank the concentration of each species (H₂A, HA¯, and A²¯) that will be present in solution at equilibrium from most to least concentrated. [H₂A] > [HA¯] > [A² −] ▼ M b. Will the solution be acidic, basic, or neutral? M acidic c. Find the equilibrium concentration of H₂A OH 0.0975 d. Find the equilibrium concentration of HA™ 2.5e-03