How do you find the charge a compound has? I'm new to chemistry, and I'm wondering how you determine what the charge of a compound is. For instance, I know that NO3 has a charge of -1. But how would I figure that out on a test? Additionally it'd be great if someone could also explain to me how to determine if something is a strong/weak electrolyte, or a non-electrolyte.

How do you find the charge a compound has? I'm new to chemistry, and I'm wondering how you determine what the charge of a compound is. For instance, I know that NO3 has a charge of -1. But how would I figure that out on a test? Additionally it'd be great if someone could also explain to me how to determine if something is a strong/weak electrolyte, or a non-electrolyte.

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter15: Solutions

Section: Chapter Questions

Problem 96AP

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You are given a 1.50-g mixture of sodium nitrate and sodium chloride. You dissolve this mixture into 100 mL of water and then add an excess of 0.500 M silver nitrate solution. You produce a white solid, which you then collect, dry, and measure. The white solid has a mass of 0.641 g. a. If you had an extremely magnified view of the solution (to the atomic-molecular level), list the species you would see (include charges, if any). b. Write the balanced net ionic equation for the reaction that produces the solid. Include phases and charges. c. Calculate the percent sodium chloride in the original unknown mixture.
The units of parts per million (ppm) and parts per billion (ppb) are commonly used by environmental chemists. In general, 1 ppm means 1 part of solute for every 106 parts of solution. Mathematically, by mass: ppm=gsolutegsolution=mgsolutekgsolution In the case of very dilute aqueous solutions, a concentration of 1.0 ppm is equal to 1.0 g of solute per 1.0 mL, which equals 1.0 g solution. Parts per billion is defined in a similar fashion. Calculate the molarity of each of the following aqueous solutions. a. 5.0 ppb Hg in H2O b. 1.0 ppb CHCl3 in H2O c. 10.0 ppm As in H2O d. 0.10 ppm DDT (C14H9Cl5) in H2O
After a student dissolved 0.5 g of white solid in water, she tested the conductivity and determined that the solution did not conduct electricity. The student then concluded: "when the white solid dissolved it 'just disappeared' so some sort of error must have been made because all solids are ionic compounds and, therefore, are electrolytes. " Comment on the student's conclusion. Is her statement a valid conclusion. If so, identify what is correct. If not, write a conclusion that would be correct.
I need help with this questions and this are the names of the substances 1.Distiled water-not electrolyte 2. Tap water- Some electrolytes 3. Sugar water- non electrolyte 4. Acetic Acid- weak electrolyte 5.NACI solution- strong electrolyte 6. sulfuric Acid- strong electrolyte name and formula of each substance concentration of each substance For each substance tested, state the conductivity record strong, weak, or nonelectrolyte formulas of ions for electrolytes or molecule for nonelectrolytes What will happen if the two electrodes come into contact with one another? Why are some substances conductive while others are not? Why does the electrode have to be cleaned each time a test is carried out? Why do some solutions light up the lower power bulb but not the higher power bulb?
A chemist needs 12.19 mL of 1.99 M NaOH. What volume in mL of 3.07 M NaOH must be diluted in water to form this solution? Please report your answer in mL to 3 sig figs.
Table sugar (sucrose) easily dissolves in water but is not an electrolyte. Is it likely that all the covalent bonds between atoms in table sugar are nonpolar bonds? Why or why not?
Chemistry Discuss whether your data in Part C (Quantitative Analysis of Salt Solutions) appears to follow a linear trend (all points near a line) or not based on your completed graph. How could you use this graph to determine the concentration of an unknown NaCl solution by just measuring the conductivity of the solution? this experiment test strong and weak electrolyte
a)Is it possible to have an ionic compound that is not water soluble?b) Is it possible for an electrolyte to be covalent?
A chemist needs 13.81 mL of 1.458 M NaCl. What volume in mL of 3.767 M NaCl must be diluted in water to form this solution?
It's worth noting that, unlike with mass, you can't just combine the volumes of the solute and solvent to get the total volume of the solution. Explain why mass is preserved when a solute and solvent are combined, but volume is not. Give a detailed explanation.
When an ionic compound such as sodium chloride (NaCl) is placed in water, the component atoms of the NaCl crystal dissociate into individual sodium ions (Na+) and chloride ions (Cl-). In contrast, the atoms of covalently bonded molecules (e.g., glucose, sucrose, glycerol) do not generally dissociate when placed in aqueous solution. Which of the following solutions would be expected to contain the greatest number of solute particles (molecules or ions)? EXPLAIN WHY THE ANSWER IS 1 LITER OF 1.0M NaCl ? STEP BY STEP
Please answer 3 and 4 1. What causes molecules to dissolve in water? What are the driving forces of solubility and how can you tell if a molecular compound will be soluble in water? 2. For each of the vitamins above, classify it as water-soluble or fat-soluble. Give your reasoning for each based on their molecular structure. 3. Suppose that a new fat-soluble vitamin was discovered. What could you say about its structure based on this information? Be sure to use the principles of molecular solubility to support your claim. 4. Suppose that a new water-soluble vitamin was discovered. What could you say about its structure based on this information? Be sure to use the principles of molecular solubility to support your claim. 5. In large doses, most vitamins can be toxic. Which type of vitamin must you be more careful about consuming too much of? Why?