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Hair Loss and Treatment
What is an anhydrate?
Asked in Chemistry
How does hydrate differ from an anhydrous compound?
Asked in Geology
What kind a of rock can be formed from evaporation?
Asked in Chemistry
What do you call a hydrate that is heated strongly?
How do you find the percent water lost from a hydrate?
Asked in Chemistry
Reaction when the anhydrous salt samples were treated with the liquid?
Usually, when a salt anhydrate is treated with water, its crystalline structure will reappear. Many solids are crystalline when the water of hydration, or water of crystallization is present. If you vaporize this away with heat, the crystalline structure collapses and you are usually left with a powdery anhydrate. Add water and it re-crystallizes. Be careful though: adding the water back will also release the heat you put into it to remove it. So adding the water is an exothermic process.
How to find the percent of water in a hydrate?
1. Find the molar mass of the hydrate. Find the molar mass of the water molecules (18.01528 x # water molecules) and of the anhydrate; add the values together to find the molar mass of the hydrate. Molar Mass Water + Molar Mass Anhydrate = Molar Mass Hydrate 2. Find the percent of water in hydrate. Divide the molar mass of water by the molar mass of hydrate; multiply by 100%. - Mass water Mass hydrate x 100%
Asked in Elements and Compounds, Chemical Bonding
What are hydrates and what is hydration?
Some salts have a property called "hygroscopy". This means that they absorb water from the air in a preset ratio (like, 5 molecules of water for every 2 units of the salt for example). They give this water off when heated. Therefore, there are actually two forms of the salt, they "hydrate" or "hydrous" form, which has the water, and the "anhydrate" or "anhydrous form", which does not. These two forms can have surprisingly different properties. Hydration is the process of going from an anhydrate to a hydrate (the source of the water doesn't matter, so don't say it's "absorbing water from the air").
How do you calculate percent water lost in hydrate?
1. Find the amount of water lost. Subtract the mass of the anhydrate (substance after it's been heated [meaning no water left]) from the mass of the hydrate (substance before it's been heated [meaning water is present]). Water lost = mass hydrate - mass anhydrate (mass before - mass after). 2. Find the percent water lost in hydrate. Divide the amount of water lost by the mass of the hydrate; multiply result by 100%. - water lost mass hydrate x 100%
What are some examples of words that use the prefix an?
Asked in Chemistry
What is the theoretical percentage of water of hydration in cacl2-2h20?
1. Find the molar mass of the hydrate (Calcium Chloride Dihydrate). Find the molar mass of water and the anhydrate (anhydrate + water = hydrate); add the molar mass values of each to find the molar mass of the hydrate. Molar Mass CaCl2: 110.98g + Molar Mass H2O: 36.04g* Molar Mass CaCl2 * 2H2O: 147.01g Finding Molar Mass # atoms element A * atomic mass element A = Mass A # atoms element B * atomic mass element B = Mass B ... etc. Add up all the mass values and you have the value for molar mass. Do this for both the anhydrate and the water molecules. Add these values together to find the molar mass of the hydrate. Molar Mass Anhydrate + Molar Mass Water Molecules* = Molar Mass Hydrate * Tip: the molar mass of water for all hydrate calculations is 18.02g x number of water molecules. This number may be useful to remember on the day of the test or while doing practice problems.* 2. Calculate the percentage of water in hydrate. Divide the molar mass of water by the molar mass of the hydrate, and multiply result by 100%. 36.04g 147.01g x 100% Percent water in hydrate is 24.52%.
Asked in Chemistry
An unknown hydrate ac xH2O has a mass of 1.632 g and the anhydrous compund AC has a mass of 1.008 g What is the experimental percentage of water in the hydrate?
Asked in Chemistry
A 6.88 g sample of the hydrated crystal Rb2CO3 xH2O is heated until all the water is removed The remaining solid weighs 5.24 g Calculate the formula of the hydrated crystal?
Okay, the anhydrate that weighs 5.24g (after heating) is pure rubidium carbonate (Rb2CO3) so the 6.88g represents the molar mass of the hydrated crystal. Set up an algebraic direct proportion: 6.88/x = 5.24/(molar mass of Rb2CO3) which is 231g/mol. Solve for x to get 303.3. Subtract out the anhydrate mass: 303.3 - 231 = 72.3. Now divide that number by water's molar mass, which is 18g/mol: 72.3/18 = 4, so the formula of the hydrate crystal is Rb2CO3-4H2O.
Asked in Acids and Bases
Suppose 5.0 g of salicylic acid is heated with an excess amount of acetic acid. What is the expected yield of acetylsalicylic acid?
Calculate The percent Water In CoC2H3O22 x 4H2O?
1. Find the molar mass (MM) of the hydrate (cobalt acetate tetrahydrate). MM Co(C2H3O2)2: 177.02g (anhydrate) + MM 4H2O: 72.06g (water) MM Co(C2H3O2)2 * 4H2O = 249.08g (hydrate) 2. Find the percent water of hydrate. Divide the mass of water by the mass of hydrate (anhydrate + water = hydrate). 72.06g 249.08g x 100% Percent water of hydrate is 28.93%. Finding Molar Mass # atoms Element A * Atomic Mass Element A = Mass A # atoms Element B * Atomic Mass Element B = Mass B ... etc. Add up all of the mass values and you have the molar mass of the substance.
What is another name for mummify?
Asked in Chemistry
How do you calculate hydrates?
It's not too hard: take a sample of a hydrate and get a really accurate mass for it. Then, stick your sample in a test tube and heat it up until it changes color completely (usually it will turn white.) This means all the water of hydration (sometimes called water of crystallization) has vaporized. Now, get another good accurate mass for the anhydrate. Work out the ratio of masses, and do a little stoichiometry with the molar mass of water (18 grams/mole.) You should end up with a certain number of moles of water per moles of substance. Copper(II) sulfate is an easy one to do. When you do all the math, you end up with a ratio of 5 moles of water to every 1 mole of anhydrate, so the formula for copper(II) sulfate hydrate works out to be: CuSO4-5H2O.
What are the formulas involving hydrates?
CALCULATING MASS OF WATER LOST IN HYDRATE To calculate how much water was lost after a hydrate's been heated, subtract the mass of the anhydrate (after) from the mass of the hydrate (before). Mass Hydrate - Mass Anhydrate = Mass Water Lost EXPERIMENTAL VALUE PERCENT WATER IN HYDRATE To calculate the experimental percent of water in a hydrate (using values gathered during the experiment), calculate how much water was lost (see "CALCULATING MASS OF WATER LOST" above). Do this by dividing the mass of the water lost (g) by the mass of the hydrate. Multiply the result by 100%. mass water lost - mass hydrate x 100% THEORETICAL VALUE PERCENT WATER IN HYDRATE To calculate the theoretical percent of water in a hydrate (using molar masses of substances rather than actual masses from experimental data), divide the molar mass of the water molecules by the molar mass of the hydrate; multiply the result by 100%. - Molar mass water Molar mass hydrate x 100% Finding Molar Mass # atoms element A * atomic mass element A = Mass A # atoms element B * atomic mass element B = Mass B ... etc. Add up all the mass values and you have the molar mass. Do this for both the anhydrate and water. For water's molar mass, you can also multiply 18.02 by the number of water molecules there are. This is a useful number to remember in order to save time test day and while doing homework practice problems too. To find the molar mass of the hydrate, add the molar mass values for water and the anhydrate. Molar Mass Water Molecules + Molar Mass Anhydrate = Molar Mass Hydrate PERCENT ERROR WATER IN HYDRATE In order to determine the percent error of the water in a hydrate, subtract the experimental value (what you determined using values found via experimentation) from the theoretical value (what is determined using molar masses), then divide value by the theoretical value; multiply result by 100%. Theoretical Value - Experimental Value x 100% ----------- Theoretical Value EMPIRICAL FORMULA OF HYDRATES(looking for quantity of water molecules) In order to find how many water molecules there are within a hydration (finding the empirical formula for hydrate), follow the steps below according to what is given. 1. Calculate percent water in substance. Divide the mass of water by the mass of the hydrate (before heating). - mass water* mass hydrate * see "CALCULATING MASS OF WATER LOST IN HYDRATE" above. Sometimes this number is already given. If it is, then proceed to the next step. 2. Convert Mass to Moles. Divide the mass of substance by its molar mass. --------- Mass substance (g) Molar mass substance (g/mol) = mol Conversion Factor mass substance (g) x 1 mol substance ----------------- atomic mass substance (g) = mol substance Do this for both the anhydrate and water. 3. Find Mole Ratio; Multiply the number of moles until they are a whole number. Find the mole ratio by dividing the number of moles for each substance by the smallest number of moles within the compound. ------- # mol anhydrate smallest # moles compound --------- # mol water smallest # moles compound AND/OR -- mol H2O mol hydrate = mol H2O per mol anhydrate Multiply or are within <0.1 from being a whole number (then just round up). This is not necessary if all the moles values are already whole numbers or are within <0.1 from being whole numbers. Whatever value is used to get a non-round number to become a round number must also be the SAME number used to multiply the round mole value(s). If you enjoy algebra, you can also do the following (solving for x): 18.02x/(18.02x + mass anhydrate) = % mass by water where x = number of water molecules.
Asked in Biology, Chemistry, Genetics
Describe the role of water in a dehydration reaction?
Water will be a product in a dehydration reaction. For example, when copper(II) sulfate hydrate is heated, the water of crystallization vaporizes, leaving behind copper(II) sulfate anhydrate. The equation is: CuSO4.5H2O --> CuSO4 + 5H2O Likewise, during dehydration synthesis (which is how more complex sugars are formed from simple sugars), sucrose can be formed from a glucose molecule and a fructose molecule. The equation is: C6H12O6 (glucose) + C6H12O6 (fructose) --> C12H22O11 + H2O
What causes the body to make to much creatine?
If it is your body, you may have a kidney problem, or the beginnings of one. A high nitrogen level in the blood can cause the creatinine level to elevate. Creatinine is an anhydrate of creatine. Notice the difference in the spelling of the two.Creatine is an alkaloid or amino acid present in muscle tissue.Creatinine is excreted by the urine.A urine test along with a blood test determines if the kidneys are functioning properly. Anabolic steroid use will elevate creatinine levels, but many other drugs can do the same. If you are using any medications, legal or not, you may want to increase your intake of water. If unprescribed, you may want to discontinue use until your levels return to normal.