emist needs to determine the concentration of a sulfuric acid solution by titration with a standard sodium hydroxide ion. He has a 0.1488 M standard sodium hydroxide solution. He takes a 25.00 mL sample of the original acid solution and es it to 250.0 mL. Then, he takes a 10.00 mL sample of the dilute acid solution and titrates it with the standard solution. endpoint was reached after the addition of 14.11 mL of the standard solution. What is the concentration of the original ric acid solution?

Solid potassium hydroxide is slowly added to 150 mL of a 0.0614 M silver acetate solution. The concentration of hydroxide ion required to just initiate precipitation is ______ M.

You collected the following data from a titration experiment using a 0.118M standardized NaOH solution to titrate a 26.65 mL solution with an unknown Molarity concentration (M) of sulfuric acid (H2SO4). Find molarity   Initial Burette Reading (mL) Final Burette Reading (mL) Vol Delivered (mL) Molarity Trail #1 0.15 19.47 19.32 ?

Each row of the table below describes an aqueous solution at 25 °C. The second column of the table shows the initial components of the solution. • Use the checkboxes in the third column to explain the type of the initial solution. The fourth column describes a change in the solution. • Use the fifth column to predict how the change in the solution will change its pH. solution initial components initial type (check all that apply) change O acidic A H₂O basic add H Cl O neutral acidic B H₂O, HI basic add NaOH O neutral acidic C H₂O, HI basic add NaI neutral acidic effect of change on pH (check one) O pH higher O pH lower O pH the same O pH higher O pH lower O pH the same O pH higher O pH lower O pH the same O pH higher D H₂O basic add K Cl O pH lower O neutral O pH the same

5mL of 0.150 M ammonia (NH3) is titrated with 0.100 M hydrochloric acid (HCl) The Kb for ammonia is 1.75 x 10-5  1)Write a balanced chemical equation for the reaction of ammonia and hydrochloric acid and a balanced chemical equation for the equilibrium of ammonia in water. 2) What is the pH of the ammonia solution prior to the addition of any HCl?

An HCl solution has a concentration of 0.09714 M. Then 10.00 mL of this solution was then diluted to 250.00 mL in a volumetric flask. The diluted solution was then used to titrate 250.0 mL of a saturated AgOH solution using methyl orange indicator to reach the endpoint. 1. What is the concentration of the diluted HCl solution?   2. If 7.93 mL of the diluted HCl solution was required to reach the endpoint, what is the concentration of OH− in solution?   3. What is the concentration of Ag+ in solution?

you would like to remove cadmium ions from a waste stream using precipitation. The final concentration of cadmium needs to be less than 0.001 mg/L. identify a chemical that could be used to precipitate cadmium out of solution to meet this goal. Show calculations and prove if it can be calculated.

3a) A student determines the concentration of a sodium hydroxide solution by titration with standardized KHP. S/he obtains the values: 0.190 M, 0.202 M, and 0.205 M. Should the value 0.190 M be rejected? Apply the Q Test. For three values Q must be greater than 0.94 to reject the number. Q = suspect nearest | largest - - smallest b) The student de to repeat the experiment two more The five values now include: 0.190 M, 0.202 M, 0.205 M, 0.201M and 0.203M. Use the Q Test to see if the first value may be rejected. For five values Q must be greater than 0.64 to reject the number. c) Solve for the average Molarity of the measurements from part b with and without the rejected number. Is there value in repeating an experiment several times?

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Calculate the molarity of an NaOH solution from the following titration data.  Be sure the answer has the correct amount of significant figures.  The chemical equation for this titration is as follows: NaOH  +  KHP  ⟶  NaKP  +  H2O NaOH buret reading, inital:  15.27 mL NaOH buret reading, final:     8.32 mL Mass of KHP (204.22 g/mol):  1.1592 g Calculate the molarity of an NaOH solution from the following titration data.  Be sure the answer has the correct amount of significant figures.  The chemical equation for this titration is as follows: NaOH  +  KHP  ⟶  NaKP  +  H2O NaOH buret reading, inital:  15.27 mL NaOH buret reading, final:     8.32 mL Mass of KHP (204.22 g/mol):  1.1592 g