Please don't provide handwritten solution ... Calculate the solubility of silver chloride in a solution that is 0.170 M in NH3 (initial concentration). Express your answer using two significant figures.

Will the calculated Molarity of NaOH be too high or too low or unaffected if the following happen: When you answer the question, consider how the situation affects the calculation of molarity of NaOH and moles NaOH, which is calculated from the mass of KHP. For each answer, you must supply a clear explanation for your answer. Often times, students will restate the facts rather than explaining why they chose the answer they chose. a) You add the weighed KHP to a flask containing a 60mL of water rather than 50 mL of water. Explain. Your answer must contain a well-thought-out and clearly written explanation. b) The buret is still wet with water on the inside when you add your NaOH solution. Explain c) The KHP is wet when you weigh it. Explain. d) You titrate past the equivalence point by 0.50mL Answer a-d

Note:- • Do not provide handwritten solution. Maintain accuracy and quality in your answer. Take care of plagiarism. • Answer completely. • You will get up vote for sure.

40 ml of a 0.100 M sodium phosphate solution is mixed with 40 ml of a 0.200 M cobalt (II) nitrate solution, generating a fine purple solid. The solid is removed via filtration and the liquid is saved.  Given that nitrate compounds are always soluble and phosphate compounds are generally insoluble, what chemical species are present in the precipitate and in the supernatant? Explain your answer.

Solid zinc nitrate is slowly added to 175 mL of a 0.0572 M potassium sulfide solution. The concentration of zinc ion required to just initiate precipitation is  M.

Subject: chemistry

True or false: the determination of a molar mass of a compound by the titration method used today depends on having a pure sample of the unknown compound? Explain.

Use the data below to determine the % by mass of Fe to TWO decimal places, if a 0.019 M KMnO4 solution was used for the titration. (MM Fe = 56 g/mol) mass of iron compound (g) 0.637 initial buret reading (mL) 0.86 16.60 final buret reading (mL) Type your answer...

A chemistry student weighs out 0.0852 g of phosphoric acid (H,PO,), a triprotic acid, into a 250. mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.1500 M NaOH solution. Calculate the volume of NaOH solution the student will need to add to reach the final equivalence point. Be sure your answer has the correct number of significant digits. mL

b) The solubility rules provide a qualitative assessment of what combination of ions will form a precipitate when mixed in water. However, what general statement can be made regarding the solubility of all ionic compounds? Why? c) Explain why gases dissolve less in solution when the solution is heated?