Since HCl is a strong acid which completely ionized.
Therefore, [HCl] = [H+] = 0.0036M
pH = -log[H+] = -log[0.0036]
pH = 2.44
pH + pOH =14
pOH = 14 - pH = 14 - 2.44
pOH = 11.56
Please use the values in the resources listed below instead of the textbook values. what are...
Please use the values in the resources listed below instead of the textbook values. The pH of 0.50 M solution of Hris 1.76. Determine K, for HF from these data (Assume K -1.0110 ) Supporting Materials Periodic Table Supplemental Data Constants and Factors Additional Materials Section 14,3 Submit Answer Practice Another Version -/10 points OSGENCHEM1 14.3.P.076. | о му The pH of a 0.125 mM solution of the alkaloid yohimbine is 8.76. Determine K for yohimbine from these data. (Assume...
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my Nules || Ask Your Teac The concentration of hydroxide ions in an aqueous solution is 3.8x109 M. What is the concentration of hydronium ions in this solution at 25°C? M Need Help? 2. - 3 points WAS OSGENCHEM1 14.1.WA.017. My Notes Ask Your Teache Calculate the concentration of the hydroxide ion (OH) in an aqueous solution if the hydronium ion (H20) concentration is 4.98 x 10 Kw - [H,0*1(OH) - 1.01x10-14 at 25°C. moll mol/L. The lon-product constant for...
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NAME: 1 Fill in the blanks with the appropriate value. Please express concentration values to 3 significant figures. Dont forget the appropriate units (M) for [H3O+] and [OH-], where necessary. In addition, express pH and pOH values to two decimal places. a) [H3O+] = 1.00 x 10-'M [OH-]= pH = POH= b) [H3O+]= [OH-]= pH=2.00 POH= c) [H3O+]= [OH-] = 8.57 x 10-3 M pH = pOH = d) [H3O+]= [OH-]= pH= POH= 10.47 2 Label the above solutions as...