Which of the following solutions would have an acidic pH at 25 deg ?
X. FeBr3(aq) Y. CH3NH3Cl(aq) Z. NaNO2(aq)
A. X only
B. X and Y only
C. Y only
D. Z only
E. X and Z only
Which of the following solutions would have an acidic pH at 25 deg ? X. FeBr3(aq)...
Which of the following 0.10M solutions have pH > 7? W. NH4I X. BaCl2 Y. KNO3 Z. NaF A. W only B. Z only C. Y and Z D. W and X E. X and Y
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...
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
Which of the following solutions would have the lowest pH? Assume that they are all 0.10 M in acid at 25∘C. The acid is followed by its Ka value. A. A) HF, 3.5 × 10-6 B. B) HCN, 4.9 × 10-10 C. C) HNO2, 4.6 × 10-5 D. D) HCHO2, 1.8 × 10-4 E. E) HClO2, 1.1 × 10-2 F. F) none of these
Which of the following solutions is the most acidic? Which has the lowest pH? A. 1.0 M HCl B. .01 M HCl C. 1.0 M CH3COOH D. .01 M CH3COOH
What is true about the following reaction at 25°C?<br /> HBrO(aq) + NaCl(aq) = NaBrO(aq) + HCl(aq) OK> 1 hence there will be mostly products at equilibrium. OK> 1 hence there will be mostly reactants at equilibrium. OK< 1 hence there will be mostly products at equilibrium. OK< 1 hence there will be mostly reactants at equilibrium. Question 8 (1 point) Which of the following would be more soluble in an acidic solution?<br />i. LiBr(s)<br /> ji. KNO3(s) O both...
An amino acid would have the following structure under which of the following conditions? a. neutral solution b. basic solutions c. acidic solution d only at pH 6.5
Which of the following solutions would require the quadratic equation to calculate the pH without a substantial error? A. 0.10 M HCl(aq) B. 0.10 M CH3COOH (aq), Ka(CH3COOH) = 1.8 x 10−5 C. 0.10 M KCN(aq), Ka(HCN) = 4.9 x 10−9 D. 0.10 M KHSO4(aq), Ka(HSO4–) = 1.3 x 10−2
Complete the following table. (All solutions are at 25 ?C.) [H3O+] [OH?] pH Acidic or Basic _____ _____ 3.15 _____ 3.7
Which of the following solutions would have the highest pH? Assume that they are all 0.10 M in acid at 25 C. The acid is followed by its Ka value. HC102, 1.1 x 10-2 OHCHO2, 1.8 x 10-4 HC6H50, 1.3 * 10-10 O HNO2, 4.6 x 10-4 O HOCI, 2.9 x 10-8