Determine the pH
1. [H3O+]=9.0×10^−9M
![Hydrogen ion concentration[H0] =9.0x10°M pH = - log[H:0] =- log(9.0x109) = 9.0- log(9.0) =8.05 Hence, pH of the solution is](http://img.homeworklib.com/questions/d1fbe090-6f56-11ec-849f-bb9e255ee90b.png?x-oss-process=image/resize,w_560)
Determine the total alkalinity in mg CaCO3/L given the following: a)[HCO3-] =0M ,[Co3^2-]=0M ,[OH-]=1.0*10^-5M ,[H3O+]=1.0*10^-9M b)[HCO3-] =0.0100M ,[Co3^2-]=0M ,[OH-]=2.0*10^-6M ,[H3O+]=5.01*10^-9M c)Convert a and b to meq. I already aksed this question once on Cheg, and it was not explaned so i am re-asking in hopes for a better responce. A step by step solution would be greatly appreciated.
For each strong base solution, determine [OH−], [H3O+], pH, and pOH. 1. 7.77×10−3 M LiOH, determine [OH−] and [H3O+]. 2. For this solution determine pH and pOH. 3. 0.0212 M Ba(OH)2, determine [OH−] and [H3O+]. 4. For this solution determine pH and pOH.
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 the [OH−] of each aqueous solution with the following [H3O+]:orange juice, 2.4×10−4M and bile, 6.0×10−9M
1) A solution has [H3O+] = 4.0×10−5 M . Use the ion product constant of water Kw=[H3O+][OH−] to find the [OH−] of the solution. Express your answer to two significant figures. Calculate the [OH−] value of each aqueous solution. 1)milk of magnesia with [H3O+]=3.0×10−9M. Express your answer using two significant figures. 2)pancreatic juice with [H3O+]=4.0×10−9M Express your answer using two significant figures. Carbonated cola is more acidic than coffee or even orange juice because cola contains phosphoric acid. What is...
1.Calculate the pH of each solution and indicate whether the solution is acidic or basic. A. [H3O+] = 1.8 x 10-4M B.[H3O-] =7.2 x 10-9M 2.Calculate the [OH-] in each solution and determine whether the solution is acidic =, basic, or neutral. A. [H3O+] = 7.5 x 10-5M B. [H3O+] = 1.5 x 10-9M C.[H3O+] = 1.0 x 10-7M 3. Write a molecular equation for the neutralization reaction between aqueous HCI and aqueous Ca(OH)2?
For each strong base solution, determine [OH−], [H3O+], pH, and pOH. 1.0×10−4 M Ca(OH)2, determine [OH−] and [H3O+]. For this solution determine pH and pOH. 2.9×10−4 M KOH, determine [OH−] and [H3O+]. For this solution determine pH and pOH.
a. [OH−]=0.002M b. [OH−]=1.2×10−4M c. [H3O+]=8.5×10−2M d. [H3O+]=4.2×10−8M Determine the pH for each
at .2M and 10 mL pH= 2.78 at .02M and 1mL pH=3.32 a) Determine the [H3O+]eq from the pH values for each solution. b) Construct ICE tables and use the initial molarity of [HC2H3O2] for each diluted solution, the equilibrium concentration for [H3O+]eq and the equation below to determine [C2H3O2–]eq and [HC2H3O2]eq. HC2H3O2(aq) + H2O (l)--> H3O+(aq) + C2H3O2–(aq) c. Write the Ka expression for the acid dissociation reaction and substitute the calculated equilibrium concentrations in to determine the Ka...
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