the pH of a solution is decreased from 9 to 8, it means that theA) concentration of H+ has decreased to one-tenth (1/10) what it was at pH 9.B) concentration of H+ has increased 10-fold (10X) compared to what it was atC) concentration of OH- has increased 10-fold (10X) compared to what it was atD) concentration of OH- has decreased to one-tenth (1/10) what it was at pH 9.E) Both B and D are correct.p

pH is a measurement that is used to specify acidity or basicity of an aqueous solution. The range of…

the pH of a solution is decreased from 9 to 8, it means that the A) concentration of H+ has decreased to one-tenth (1/10) what it was at pH 9. B) concentration of H+ has increased 10-fold (10X) compared to what it was at pl C) concentration of OH- has increased 10-fold (10X) compared to what it was at D) concentration of OH- has decreased to one-tenth (1/10) what it was at pH 9. E) Both B and D are correct.

the pH of a solution is decreased from 9 to 8, it means that the A) concentration of H+ has decreased to one-tenth (1/10) what it was at pH 9. B) concentration of H+ has increased 10-fold (10X) compared to what it was at pl C) concentration of OH- has increased 10-fold (10X) compared to what it was at D) concentration of OH- has decreased to one-tenth (1/10) what it was at pH 9. E) Both B and D are correct.

Biology (MindTap Course List)

11th Edition

ISBN:9781337392938

Author:Eldra Solomon, Charles Martin, Diana W. Martin, Linda R. Berg

Publisher:Eldra Solomon, Charles Martin, Diana W. Martin, Linda R. Berg

Chapter2: Atoms And Molecules: The Chemical Basis Of Life

Section2.6: Acids, Bases, And Salts

Problem 1C

See similar textbooks

Similar questions

The pH of black coffee is 5, and that of milk of magnesia is 10. Is the coffee twice as acidic as milk of magnesia?
I want to make a buffer solution containing 1 M glycene pH = 10 (Na+), 1 mM ZnCl2 , 1 mM MgCl2. I have the stock solutions 1 M glycene, 1 M MgCl2, 1 M ZnCl2, and 10 M NaOH. My final volume of buffer solution needs to be 250ml. how much (in ml) of each solution should i put into my buffer?
pH expresses the molar concentration of hydronium ions in an aqueous solution on a logarithmic scale. (Note that it is common to use the hydrogen ion, H*, to represent the hydronium ion, H3O+.) pH = -log[H3O+] [H3O+] = 10-PH As pH decreases, acidity increases. As pH increases, acidity decreases. • Acidic solution: pH 7 Part A - Calculating pH Submit [H₂0+] 1 Acidic pH 01 10¹ 102 103 104 105 106 107 108 109 10-10 10-11 10-12 10-13 10-14 stomach acid 3 wine lemon tomatoes juice vinegar, black soft drinks, coffee beer 6 Neutral urine milk 7 human blood pure water sea- water baking soda 10 11 12 13 14 milk of magnesia house- hold ammonia oven cleaner Basic household bleach Adapted from Biological Science by Freeman ©2008 Pearson Education, Inc. What is the pH of an aqueous solution with the hydronium ion concentration [H3O+] = 2 x 10-14 M? Make sure that your answer has the correct number of significant figures. For help determining the correct number of significant figures, see Hint 3. ►…
What is the pH of a buffer that contains 0.9 M ammonia and 0.3 M ammonium ion? (Ka for ammonium ion = 5.8 x 10-10
What is the purpose of: A. The concentrated salt solution? B. adding isopropyl alcohol to the solution? Why does it need to be in low temperature?
Suppose you wanted to make a buffer of exactly pH 7.00 using KH2PO4 and Na2HPO4. If the final solution was 0.1 M in KH2PO4, what concentration of Na2HPO4 would you need?
How much of the enzyme proteinase k (solute) is required to make 250ml of a solution with a concentration of .01mg/ml? (Weight/volume ratio)
Indicate whether a solution will have more OH- or H+if the value of the solution is 10.
In a hospital laboratory, a 10.0 mL sample of gastric juice, obtained several hours after a meal, was titrated with 0.01 M NaOH to neutral pH of 7.0; 72.0 mL of NaOH was required for this titration. The patient’s stomach contained no ingested food or drink, thus assume that no buffers were present. What was the pH of the 10.0 mL gastric juice sample before titrating with NaOH?
How much water must be added to 300 mL of an aqueous solution of 0.2 M acetic acid in order to double the degree of ionization? Take the acid ionization constant of acetic acid to be 1.8 x 10-5.
You just made a 1.5M permanganate solution. What concentration is your potassium permanganate solution in percent? "K: 39.10 g/mole" "Mn: 54.94 g/mole" "O: 16 g/mole" "MW of KMnO4 is 158.04 g/mole" O a. 0.24% Ob. 20.1% O c. 15.8% O d. 23.7% O e. 2%
Calculate the pH of the resulting solution if 23.0 mL of 0.230 M HCl(aq) is added to 33.0 mL of 0.230 M NaOH(aq). pH = Calculate the pH of the resulting solution if 23.0 mL of 0.230 M HCl(aq) is added to 13.0 mL of 0.330 M NaOH(aq). pH=