Calculate [H3O ] for the following solutions:
a) 5.29 × 10–3 M HBr
b) 1.10 x 10-2 M KOH
Calculate [H3O ] for the following solutions: a) 5.29 × 10–3 M HBr b) 1.10 x...
Calculate [H3O+] for a 3.44×10−3 M HBr solution. Calculate [H3O+] for a 1.00×10−2 M KOH solution.
6. Which of the following solutions is acidic [H3O+] = 7.0 x 10-7 M B)/ [H3O"] = 1.5 x 10-10 M C) [H3O+] < 7.0x10-7 M D) [H30]> 7.0 x 10'M E) 「HOT! = 1.0x10-14 M 25. The pH of tomato juice is about 4.5 Calculate the concentration of hydrogen ions in this juice A) 3 x 10-10 B) 3 x 10-5 M C) 5 x 104 M D) 4 M E) 3 x 1010 M
Calculate H,0*] for a 5.32 x 10-M HBr solution. H,0+1 = x10 Calculate (H,0+) for a 1.50x 10 ? M KOH solution. [H,0+) = X10 x10
Calculate the pH of each of the following solutions. 0.50 M HBr 3.1×10−4 M KOH 4.2×10−5 M Ca(OH)2
For each of the following strong base solutions, determine [OH−],[H3O+], pH, and pOH. A) 8.75*10^-3 M LiOH: [OH-] & [H3O+] B) pH & pOH C) 1.13*10^-2 M Ba(OH)2: [OH-] & [H3O+] D) pH & pOH E) 2.0*10^-4 M KOH: [OH-] & [H3O+] F) pH & pOH G) 5.1*10^-4 M Ca(OH)2 H) pH & pOH
2. Calculate the pH of the following solutions: (a) [H3O+] = 1.4 x 10-'M (b) [OH-] = 3.5 x 10-2M (c) pOH = 10.5 3. What is the pH of a 0.10 M solution of HCIO4? (A strong acid) 4. Write the dissociation reaction and the corresponding K, expression for the following acids in water. (a) H3PO4 (b) C&H OH 5. Write the reaction and corresponding Ko expression for each of the following bases in water. (a) NH3 (b) PO4...
Calculate the pH and pOH of each of the following solutions. [H3O+]= 1.5×10−8 M [H3O+]= 1.0×10−7 M [H3O+]= 2.1×10−6 M
Which of the following solutions is acidic? A. [H30+] = 7.0x10^-7 M B. [H3O+] = 1.5 x 10^-10 M C. [H3O+] <7.0 X 10^-7 M D. [H3O+] > 7.0 X 10^-7 M E. [H3O+] = 1.0 X 10^-14 I attempted this by finding pH via the negative log of each H3O value.... which gives me a pH of 6.15 when [H3O+] is 7.0 x 10^-7 M. The way the question is worded is tricky however - it seems that only...
Determine the pHfor the following solutions: Part B [H3O+] = 4.2×10−3 M Part C [H3O+]= 2×10−4M Part D [OH−]= 8.8×10−9M
Calculate either [H3O+] or [OH-] for each of the solutions at
25°C. Solution A: [OH-] = 2.67 * 10^7 M. Solution B: [H3O+] = 9.91
* 10^9 M. Solution C: [H3O+]= 0.000731 M
Solution A: [OH= 2.67 x 10- 7 M Solution A: H,O*1=|3.75 x10 M Solution B: H,O 9.91 x 10 Solution B: OH M Solution C: H,0 0.000731 M Solution C: OH Which of these solutions are basic at 25 °C? Solution A: OH =2.67 x 10 M...