117. Chemistry The pH of a chemical solution is given by the formula pH = -log 10[H*] where [H*] is the concentration of hydrogen ions in moles per liter. Values of pH range from 0 (acidic) to 14 (alkaline). (a) What is the pH of a solution for which [H*] is 0.1? (b) What is the pH of a solution for which [H*j is 0.01? (c) What is the pH of a solution for which [H*] is 0.001? (d) What happens to pH as the hydrogen ion concentration decreases? (e) Determine the hydrogen ion concentration of an orange (pH = 3.5). (f) Determine the hydrogen ion concentration of human blood (pH = 7.4).

117. Chemistry The pH of a chemical solution is given by the formula pH = -log 10[H] where [H] is the concentration of hydrogen ions in moles per liter. Values of pH range from 0 (acidic) to 14 (alkaline). (a) What is the pH of a solution for which [H] is 0.1? (b) What is the pH of a solution for which [Hj is 0.01? (c) What is the pH of a solution for which [H*] is 0.001? (d) What happens to pH as the hydrogen ion concentration decreases? (e) Determine the hydrogen ion concentration of an orange (pH = 3.5). (f) Determine the hydrogen ion concentration of human blood (pH = 7.4).

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

What is [H+] concentration if pH=0?
Solution step by step
Determine the [OH-], pH, and pOH of a solution with a [H*] of 0.014 M at 25 °C. [OH-] = M pH = pOH = Determine the [H*), pH, and pOH of a solution with an [OH] of 8.4 x 10-9 M at 25 °C. [H*] = M pH = pOH = Determine the [H*], OH], and pOH of a solution with a pH of 13.05 at 25 °C. [H*] = M [OH¯] = pOH = Determine the [H*], OH], and pH of a solution with a pOH of 13.25 at 25 °C. [H*] = M [OH-] = M pH =
[H+] = 3.865 x 10^-9 M ; calculate [OH-]
Calculate the [H+] in a solution that has a pH of 9.88.
Calculate the [OH-] in a solution with a pH of 6.59?
Nicotinic acid, HC,H&NO2, is a B vitamin. It is also a weak acid with K, = 1.4 x 10-5. Calculate [H+] and the pH of a 0.034 M solution of HCGH4NO,. [H*] = Use correct number of significant digits; pH = Use correct number of significant digits;
USE ICE TABLE TO COMPLETE
To obtain pH, you need [H*] ions. We established that [H*] = 0.010 M. Since pH = -log[H* ] ions, then what is pH? Your answer:
Calculate the pH of a solution that has a hydronium ion concentration, [H,O*], of 1.10 × 10-9 M. pH
Determine the pH of a solution with [H3o*] = 1.73 x 10-5 M. Your answer should contain 3 decimal places as this corresponds to 3 significant figures when dealing with logs. pH
a.) What is [OH−] in a solution with a pH of 9.67? b.)How much heat does your body lose when 1.6 g of sweat evaporates from your skin at 25∘C? (Assume that the sweat is only water.) The heat of vaporization of water at 25∘C is 44.0 kJ/mol. Express your answer in kilojuoles to two significant figures. c.) How many kJ of heat are needed to completely vaporize 1.30 moles of H2O? The heat of vaporization for water at the boiling point is 40.6 kJ/mole.