TEST: SOLUTIONS, ACIDS, AND BASES MULTIPLE CHOICE Select the answer that best completes the statement or that correctly answers the question. 1. The salt in water (only the solid) is the __________. a. Solvent c. Solute b. Solution d. Concentrate 2. The water in salty water (only the water) is the __________. a. Solvent c. Solute b. Solution d. Concentrate 3. A mixture of salt and water is knows as: a. Solvent c. Solute b. Solution d. Concentrate 4. What do you call a solution that contains more solute dissolved in it that it can hold at a specific temperature: a. A solution c. A concentrate b. A supersaturated solution d. an extraordinarily saturated solution 5. Which of the following is the best way to prepare a 1 molar, 1 liter, …show more content…
A solution with a pH of 7.0 is considered _______. a. Acidic c. alkaline (basic) b. Neutral d. saturated 9. If the concentration of the H+ ion is greater than the concentration of the OH- ion, the solution is said to be ________. a. Acidic c. alkaline (basic) b. Neutral d. saturated 10. If the concentration of the H+ ion is equal to the concentration of the OH- ion, the solution is said to be ________. a. Acidic c. alkaline (basic) b. Neutral d. saturated 11. What is the concentration of a solution that contains 10.0 moles of HCl in 5.50 L of water? a. 1.82 M c. 0.550 M b. 15.5 M d. 4.50 M 12. A beaker contains 0.7 L of a 2 M calcium carbonate solution. If enough water is added to reach a final volume of 0.80 L, what is the solution’s new concentration? a. 2.23 M c. 1.75 M b. 1.12 M d. 0.28 M 13. What is the [OH-] in water if its [H+] = 1 x 10-6? a. 1.0 × 10-20 M c. 1.0 × 1020 M b. 1.0 × 10-8 M d. 1.0 × 108 M 14. A solution has a pH of 3.5 (pH = 3.5). What is its H+ concentration? a. 3.16 × 10-8 M c. 3162 M b. -0.544 M d. 0.544 M 15. A solution has an H+ concentration of 0.03 M ([H+] = 0.03). What is its pH? a. 1.52 c. -1.52 b. 0.933 d. 1.07 KEY 1. C 2. A 3. B 4. B 5. C 6. B 7. C 8.
5. Question 5: a) As mentioned in the manual, we have the ratio (K/H+ ), if H+ was lower than K then the equivalent point will be achieved and it will change color. And if H+ was more than K then the solution we are titrating will be the same, the equivalent point won’t be achieved, and it will be acidic solution. And to find the value of H+ is by having the value of pH, therefore the pH has changed from 7 to 9, which is by shifting from 10-7 to 10 -8 by adding the 0.01 of the base, and it will shift again from 10 -8 to 10 -9 by adding another 0.01 of the base to the solution , the different that’s added between the two shifting are close to each other which indicates that the
Data: Water: Chart 1 pH Average ±
1b. The author has chosen to write to a fairly narrow audience. Those reading the article are likely to side with the opposing
This is the best answer choice because it shows opposite things in parallel structure like often and seldom. 19.D. This question asks about why the provided sentence is in quotation marks. D is the best answer choice because he seems to be trying to make clear his major claim. 20.
I organized four different tests; pH paper, alkalinity tests, the number of rocks neutralizing acid, and the number of rocks that don’t neutralize acid. The average for pH paper was seven. The pH is the numeric scale used to specify the acidity or alkalinity of an aqueous solution. The pH scale measures acidity and alkalinity. the pH scale goes from zero, which is an acid reading, to fourteen, which is an alkaline reading.
= 10^-3 M = 1,000 mL Here C1,C2; are the first and second concentrations of solution V1 and V2 ; are the required and current volumes. The impeller turned on and DDA, and tap water left to be mixed properly with water for 2 minutes. Approximately 150 grams of quartz added into the solution.
Equivalence Point: pH at which the moles of H3O¬+ equal the moles of OH- and solution is neutralized. Indicator: A weak acid or base and its conjugate ion whose color changes as pH
Salt: Q1: What is salt? Salt, otherwise referred to as sodium chloride, is an exceedingly common mineral that is known for its strong flavour and crystalline appearance. Because of this, salt is routinely used in the preparation, preservation, and seasoning of foods the globe over (though the latter purpose is by far the one most commonly utilised), as it has been for generations.
(0.01 moles of NaOH) x (1 mole Ca(OH)2/ 2 moles of NaOH) = 0.005 moles of Ca(OH)2 Tube 1: (0.0020 moles of CaCl2) x (1 mole Ca(OH)2/ 1 mole of CaCl2) = 0.002 moles of Ca(OH)2 (0.002 moles of Ca(OH)2) x (74.08 grams/mole) = 0.1 grams = theoretical yield Tube 2: (0.0035 moles of CaCl2) x (1 mole Ca(OH)2/ 1 mole of CaCl2) = 0.004 moles of Ca(OH)2 (0.004 moles of Ca(OH)2) x (74.08 grams/mole) = 0.3 grams= theoretical yield Tube 3 (0.0050 moles of CaCl2) x (1 mole Ca(OH)2/ 1 mole of CaCl2) = 0.005 moles of Ca(OH)2 (0.005 moles of Ca(OH)2) x (74.08 grams/mole) = 0.4 grams =theoretical yield Tube
Acids are proton donors in chemical reactions which increase the number of hydrogen ions in a solution while bases are proton acceptors in reactions which reduce the number of hydrogen ions in a solution. Therefore, an acidic solution has more hydrogen ions than a basic solution; and basic solution has more hydroxide ions than an acidic solution. Acid substances taste sour. They have a pH lower than 7 and turns blue litmus paper into red. Meanwhile, bases are slippery and taste bitter.
Strong acids and strong bases are strong electrolytes and are assumed to ionize completely in the presence of water. Weak acids however, only ionize to a limited extend in water. Any weak or strong acids when in contact with any weak or strong alkali will start to undergo neutralization regardless of their volume. When an indicator which is present in the acid-base mixture and have experienced colour change, it indicates that the mixture is in right proportions to neutralize each other and is also known as the equivalence point.
It is an outstanding commodity due to its abundance and distinctive structural properties (Eckardt,2003). And some animals can digest cellulose with the help of symbiotic micro organisms that may live in their guts (Somerville,2006). Aqueous solution is a solution which solvent is water. It is usually shown chemical equation relevant to the chemical formula. It is used to determined whether the match can attract forces.
Therefore, this experimentation indicated that the sucrose molecules cannot diffuse from the concentration of the dilute solution, while on the other hand the water molecules diffuse from the dilute solution to the concentrated one. Hypothesis: If the (independent variable) sucrose of the dilute solution is
Solubility of a Salt Introduction: The solubility of a pure substance in a particular solvent is the quantity of that substance that will dissolve in a given amount of a solvent. Solubility varies with the temperature of the solvent. Thus, solubility must be expressed as quantity of solute per quantity of solvent at a specific temperature. For most ionic solids, especially salts, and water, solubility varies directly with the temperature.