a solution formed by dissolving an antacid tablet has a pOH of 4.48 calculate [H+]
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a solution formed by dissolving an antacid tablet has a pOH of 4.48 calculate [H+]
4. A student analyzed an antacid tablet from a bottle of 48 tablets purchased at a discount store for $1.00. The mass of the tablet was 1.462g. After adding 25.00mL of 0.8000/M HCl solution to the tablet, the student back-titrated the excess HCI with 3.52 mL of 1.019M NaOH solution. (a) Calculate the number of moles of HCI added to the tablet (b) Calculate the number of moles of NaOH required for the back-titration (c) Calculate the number of moles...
(1) A student is given an antacid tablet that weighs 5.4320 g. The tablet is crushed and 4.1220 g of the antacid is added to 200. mL of simulated stomach acid. It is allowed to react and then filtered. It is found that 25.00 mL of this partially neutralized stomach acid required 14.4 mL of a NaOH solution to titrate it to a methyl red end point. It takes 27.8 mL of this NaOH solution to neutralize 25.00 mL of...
For the antacid TUMS how do you calculate the mass of inert binder in a tablet, and the mass perecnt of inert binder? Tablet 1 net mass of the tablet is 1.32 g calculated mass of active ingredient is 569 mg millimgrams of active ingredient by manufacturer is 500mg % of relative difference is 13.8%
The label on an antacid product states that one tablet contains 295.0 mg of CaCO3. Calculate the volume of 0.1750 M HCl that one tablet will neutralize during a back-titration. Remember to consider the balanced reaction equation between HCl and CaCO3.
Suppose a student adds 25.00 mL of 0.989 M HCl to a 1.54 g antacid tablet. The student uses 21.1 mL of 0.543 M NaOH to titrate the solution. Calculate the moles of acid neutralized per grams of tablet. __________mol/g
The active ingredients in a particular antacid tablet are aluminum hydroxide Al(OH)3, magnesium hydroxide Mg(OH)2 and an inert "binder". A 500 mg sample of the active ingredients was dissolved in 50.0mL of 0.500 M HCl. The resulting solution, which was still acidic required 30.9 mL of 0.255M NaOH for neutralization. (a) Calculate the number of OH ion moles in the antacid tablet. (b) If the antacid tablet contains 5.0% (mass) of the inert "binder" , how many milligrams of aluminum...
In this question you will calculate the [H,0], [OH1, pH, and pOH of a solution made by dissolving 0.400 g of the strong base Ca(OH)2 (calcium hydroxide) in enough water to make 500.00 mL of solution? We will proceed in steps. a) Calculate the molarity of this solution of Ca(OH)2 >For full credit, show the steps you used to obtain your answer b) Write a balanced equation for the dissolution of Ca(OH)2 in water. (2
Calculate the [H+], the [OH-], the pH and the pOH for a solution prepared by diluting 50.0 ml of 0.035 M HNO3 to 250 ml in a volumetric flask
pOH = Determine the (H+), (OH), and pOH of a solution with a pH of 10.18 at 25 °C. [**=( (OH) = pOH = Determine the (H). OH"], and pH of a solution with a pOH of 10.71 at 25 °C. [H]= [OH-] = pH =
"Milk of magnesia" antacid has a pH of 10.25. What is the [H+] in this solution? A. 5.6 × 10-11 B. 1.8 × 1011 C. 1.8 × 10-4 D. 3.75 E. 1.8